Preliminary  Study  of  the 
Waters  of  the  Jemez  Plateau, 
New  Mexico 


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OF 

THE  UNIVERSITY 
OF  CALIFORNIA 

LOS  ANGELES 


The  RALPH  D.  REED  LIBRARY 

DEPARTMENT  OP  GEOLOGY 
UNIVERSITY  of  CALIFORNIA 

LOS  ANGELES.  CAUF. 


Bulletin  University  of  New  Mexico 


WHOLE  NUMBER  71 


Chemistry  Series  _.__._  Vol  I,  No.   1. 


A  PRELIMINARY  STUDY  OF  THE  WATERS 
OF  THE  JEMEZ  PLATEAU,  NEW  MEXICO 

-BY- 

Kelly  and  E.   V.   Anspack 
'      Class  of  1913 


ALBUQUERQUE,  NEW  MEXICO 

SEPTEMBER,  1913 


Published  quarterly  by  the  University  of  New  Mexico 

Entered  May   1,   1906,  at  Albuquerque,   N.  M.,  as  second  class  matter 

under  Act  of  Congress  of  Ju!y  16,  1894 


Geology 
Library 

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0  C 
L(o 


Bulletin  University  of  New  Mexico 


WHOLE  NUMBER  71 


Chemistry  Series  -          -          -          -          -          -  Vol  I,  No.   1. 

Albuquerque,  N.   M.,   September,    1913 


A  PRELIMINARY  STUDY  OF  THE  WATERS 
OF  THE  JEMEZ  PLATEAU,  NEW  MEXICO, 

-BY- 

Clyde  Kelly  and  E.   V.  Anspack 
Class  of  1913 


INTRODUCTION. 

The  region  to  which  the  name  "Jemez  Plateau"  is 
applied  in  this  paper  is  situated  in  the  northwestern 
part  of  New  Mexico.  It  extends  from  a  point  almost 
clue  west  of  the  city  of  Santa  Fe  -northward  to  the 
Colorado  line,  a  distance  of  about  ninety  miles.  Its 
breadth  at  its  widest  part  is  about  sixty  miles.  The 
plateau  is  divided  unequally  by  the  Rio  Chama  which 
flows  through  it  from  the  northwest  to  the  southeast. 
The  southern,  or  larger  division  is  loosely  known  as  the 
"Jemez".  The  western  limit  of  this  part  is  the  Rio 
Puerco ;  its  eastern  limit  is  the  Rio  Grande.  It  con- 
tains two  important  ranges  of  mountains,  the  Naci- 
miento  range  in  the  west,  and  the  Cochiti  mountains 


2  EJ.etin  University  if  Xew  Mexico     (Chem.  fcier.,  Vol.  1 

in  the  east.     The  highest  peak  of  these  mountains  has 
an  altitude  of  11,200  feet. 

Between  the  Xacimientos  and  the  Cochitis  there  is 
a  flat  mesa  or  table-land  of  an  altitude  of  from  7,000 
to  8,000  feet.  The  northern  part  of  this,  approxi- 
mately one-third,  is  drained  by  tributaries  of  the  Rio 
Chama.  The  southern  part  is  drained  by  the  Jemez 
river  and  its  tributaries.  The  Jemez  empties  into  the 
Rio  Grande.  It  is  in  this  southern  part  of  the  plateau 
that  the  different  groups  of  springs,  whose  waters  form 
the  subject  of  study  of  this  paper,  are  found. 

PHYSIOGRAPHY  OF  THE  JEMEZ  DISTRICT. 

The  leading  physiographic  features  of  the  Jemez 
district  are  the  mountains,  which  are  characterized  by 
their  rounded  contours,  flat  mesa  lands  cut  by  numer- 
ous canons,  and  valleys  extending  along  the  lowrer 
courses  of  the  streams.  The  whole  country  shows  the 
effects  of  having  been  extremely  broken  up  at  some 
former  time.  There  are  few  hills  in  the  region,  but 
hogbacks,  dikes,  escarpments,  and  fault  lines  are  nu- 
merous. As  a  rule  the  canons  follow  the  fault  lines. 
Along  the  lower  Course  of  the  Jemez  river,  after  it 
leaves  the  protection  afforded  by  the.  mountains,  sand 
dunes  have  been  piled  by  the  prevailing  winds. 

Mi.  Pelado,  or  "Baldy"  as  it  is  commonly  called, 
with  an  elevation  of  11,200  feet,  is  the  culminating 
point  of  the  plateau.  It  is  a  solid  mass  of  porphyry 
and  is  situated  at  the  northern  end  of  the  Cochiti  range 
ard  immediately  west  of  the  Valle  Grande  tufa  vol- 
canic region.  The  site  of  the  crater  today  is  a  level 


.\o.  1,  1913.)     Kelly  an d  Ans£ach— Jemez  Plateau  Waters  3 

area.  A  further  reference  to  Mt.  Pelado  will  be  made 
later. 

Much  of  the  upper  country  of  the  plateau  is  cov- 
ered by  tufa,  while  basalt,  usually  of  the  "malpais" 
type,  caps  and  flanks  many  of  the  lower  mesas. 

The  tributaries  of  the  Jemez  river  have  their  origin 
in  the  high  rhyolitic  plateau  of  the  Nacimienro  and 
Cochiti  mountains.  Here,  they  are  mountain  streams 
which  usually  have  water  in  them.  In  their  lower 
courses,  however,  the  water  seeps  into  the  sands  and 
their  channels  are  always  dry.  On  leaving  the  moun- 
tains each  tributary  has  cut  a  deep,  narrow  canon 
varying  in  depth  from  a  few  feet  in  the  upper  part'  to 
1,200  feet  in  the  lower  course.  The  upper  part  of 
each  canon  is  cut  in  Carboniferous  rock :  the  lower 
part  is  in  the  Red  Beds  (Permian).  At  Canon  de  los 
Jeire?:,  the  Guadalupe  and  San  Diego  creeks,  having 
gathered  in  all  of  the  upper  tributaries  except  Vallecito 
creek,  unite  to  form  the  Jemez  proper.  At  this  point 
the  united  river  enters  the  site  of  an  ancient  Cretaceous 
lake. 

According  to  Reagan,  there  are  deposits  of  Jurassic- 
Cretaceous  age  in  the  area  south  of  the  Red  Beds,  and, 
as  the  dip  of  the  Carboniferous  and  Red  Bed  strata 
has  remained  unchanged,  so  far  as  direction  is  con- 
cerned since  the  Red  Bed  revolution,  it  is  probable  that 
the  streams  existed  as  far  back  as  the  Jurassic-Cretace- 
ous age  or  even  earlier. 

After  uniting  with  Vallecito  creek,  the  Jemez  con- 
tinues in  its  southward  direction  until  its  confluence 
with  the  Rio  Sab  da.  It  then  flows  eastward  along  the 


4  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

southern  limit  of  the  Plateau  and  unites  with  the  Rio 
Grande  near  the  village  of  Bernalillo. 

The  mountains  of  the  district  for  the  greater  part 
are  forested  by  pine,  fir,  spruce,  and  aspen.  None  of 
the  peaks  extend  above  the  timber  line,  although  some 
of  them  are  bare.  In  most  cases  these  barren  spots  can 
be  attributed  to  denudation  by  forest  fires. 

The  -mesas  are  rather  thinly  covered  with  pirion. 
juniper,  and  cedar,  interspersed  with  small  open  parks. 
The  valleys  produce  sage,  cactus,  and  chaparral.  In 
the  lower  valleys,  the  Mexicans  and  Indians  raise  corn. 
beans,  chili,  and  other  farm  products.  Fruit  raising  is 
also  carried  on  on  a  small  scale. 

THE  SPRINGS. 

Along  the  lower  part  of  the  Rio  Salada  and  in  the 
upper  Jcmez  river  there  are  many  springs,  some  hot. 
some  cold,  and  some  of  a  bathing  temperature.  The 
waters  of  all  of  these  springs  possess  medicinal  prop- 
erties;  and  the  principal  springs  have  been  health  re- 
sorts since  the  invasion  of  the  white  man.  These 
springs  seem  to  be  in  groups.  Tre  principal  groups 
are :  the  Sulphurs,  the  Springs  of  the  Soda  Dam  in 
the  Jemez  river,  the  Jemez  Hot  Springs  at  Perea,  the 
Indian  Springs,  the  San  Ysiclro  Springs,  and  the 
Phillip's  Springs.  These  groups  are  here  considered  in 
the  reverse  order. 

THE  PHILLIP'S  SPRINGS. 

The  Phillip's  springs  are  forty  in  number.  They 
are  situated  in  a  little  cove  between  the  granite  spur  to 
the  southwest  of  the  Nacimiento  range  and  the  Red 


Xo.  1,  1913.)     Kelly  and  Ansfach—Jemez  Plateau  Waters  *  5 

Beds  to  the  west  of  the  Jemez  on  their  western  side. 
The  space  occupied  by  them  is  not  greater  than  thirty 
acres,  though  at  an  earlier  date  their  area  was  much 
more  extensive  than  now,  as  is  attested  by  the  traver- 
tine cones  left  by  the  extinct  springs.  The  cove  occu- 
pied by  these  springs  is  about  a  mile  to  the  northeast 
of  the  Rio  Salada,  and  eight  miles  nearly  west  of. the 
Jemez  Pueblo.  The  springs  of  this  group  are  soda  or 
iron  springs.  The  soda  springs  deposit  a  cone  of  traver- 
tine around  their  mouths,  and  the  iron  springs  are  non- 
depositing.  The  springs  of  this  group  usually  have  a 
bathing  temperature ;  but  they  are  not  used  for  bathing 
purposes  on  account  of  their  isolation,  though  their  site 
would  make  an  excellent  place  for  a  health  resort. 
They  are  situated  on  the  Ojo  del  Espiritu  Santo  Land 
Grant. 

THE  SAN  YSIDRO  SPRINGS. 

The  San  Ysidro  springs  are  situated  on  either  side 
of  the  Rio  Salada  in  its  lower  course,  their  waters 
coming  to  the  surface  along  a  fault.  They  are  some 
forty  in  number.  Those  to  the  south  of  the  river  are 
bitter  magnesium,  and  those  to  the  north  are  soda 
springs.  The  waters  of  the  springs  are  cold.  They 
have  medicinal  properties;  and  throughout  the  sum- 
mer months  the  Mexicans  bathe  in  them.  These 
springs,  being  on  salt  lands,  belong  to  the  University 
of  Xew  Mexico,  because  all  the  salt  lands  of  the  state 
have  been  reserved  for  the  benefit  of  that  institution. 

Loew,  in  "Analysis  of  Mineral  Springs,"  Volume 
III  of  the  U.  S.  Geographic  Surveys  of  the  Territories, 


(j  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

gives  the  analysis  of  waters  from  these  springs  as  fol- 
lows: 

Specific  Gravity   1.0023 

The  mineral  matter  in  100  parts  of  water : 

Carbonate  of  sodium „ 0.3072 

Sulphate  of  soda 0.1639 

Carbonate  of  lime 0.0670 

Carbonate  of  magnesia 0.0243 

Carbonate  of  iron 0.0008 

Potassa        ] 

Lithia  \ traces 

Silicic  acid  J 

0.5632 

THE  INDIAN   SPRINGS. 

These  springs  extend  in  an  east  and  west  direction 
in  a  narrow  belt  of  land  about  a  mile  to  the  north  of 
the  village  of  San  Ysidro.  At  their  west  end  they 
extend  along  a  fault ;  and  it  is  probable  that  the  east- 
ern springs  of  the  group  are  also  the  result  of  a  fault. 
In  the  eastern  part,  the  fault,  if  present,  is  covered  by 
later  deposits.  The  springs  are  alkaline  but  do  not 
deposit  sinters.  They  are  cold  in  the  west  but  in- 
crease in  temperature  toward  the  eastern  part  of  the 
I .elt.  The  temperature  of  the  eastern  springs,  those  to 
the  east  of  the  Jemez  river,  is  about  120  degrees  Fah- 
renheit. They  are  being  covered  continually  with  de- 
bris brought  down  by  an  eastern  arrbyo  and  must  be 
dug  out  when  used.  The  Indians  use  these  springs 
almost  continually  during  the  summer  months ;  even 
the  Isleta  Indians,  south  of  Albuquerque,  come  here 


X  O.  1 ,  1 9 1 3 . )     Kelly  and  A  nsfiach— Jemez  Plateau  Waters  7 

to  bathe  for  their  ailments.    The  springs  are  on  Indian 
lands,  whence  the  name. 

THE   JEMEZ    HOT   SPRINGS. 

The  Jemez  hot  springs,  or  "Ojos  Calientes,"  as  the 
Mexicans  call  them,  are  situated  in  the  Jemez  river 
bed  in  Canon  San  Diego  at  Perea.  The  site  is  a  beau- 
*i  fully  picturesque  one.  The  Red  Bed  walls  of  the 
canon  rise  1,200  feet  on  either  side  of  the  river,  while 
in  the  valley,  a  little  above  the  springs,  are  the  ruins  of 
the  Indian  village  of  San  Juan  de  los  Jemez  and  of  the 
Spanish  Catholic  church  and  fortifications  of  the  first 
occupation  of  the  Spania'rds. 

These  springs  are  located  geographically  in  two 
groups.  At  each  group  are  built  comfortable  bath 
houses  and  sweating  rooms.  Hotels  have  been  erected 
for  the  benefit  of  health  seekers.  A  daily  stage  runs 
between  the  springs  and  Albuquerque.  The  springs 
are  known  throughout  America  and  in  Europe  and 
occasionally  one  meets  a  foreigner  here. 

THE   SPRINGS   OF   THE   SODA   DAM. 

The  Soda  Dam,  which  lies  about  a  mile  above  the 
Jemez  Hot  Springs,  is  a  travertine  ridge  built  directly 
across  the  Jemez  river.  It  is  about  three  hundred 
feet  long,  fifty  feet  high  at  its  highest  part  near  the 
east  end,  fifty  feet  wide  at  the  base,  and  twenty-five 
feet  wide  at  the  top.  The  river  was,  at  one  time,  com- 
pletely dammed  by  the  Soda  Dam,  but  later  it  cut  its 
way  around  the  east  end,  and  today  flows  over  the 
dam  underneath  a  large  dome,  which  has  been  built 
out  over  the  river  by  the  deposits  of  a  spring  on  top  of 
the  clam. 


g  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

In  the  American  Geologist,  Volume  31,  Reagan 
states  that  there  were  twenty-two  springs  situated  on 
the  dam  in  1902.  While  there  are  indications  of  many 
recent  active  springs  on  top  of  the  dam,  the  authors 
were  unable  to  find  more  than  half  this  number  when 
they  visited  the  region  in  1912. 

All  the  springs  deposit  travertine  and  their  waters 
running  over  the  dam  cause  the  cap  of  the  dam  to  be 
built  farther  up  and  out  each  year,  thus  leaving  rooms 
beneath  the  cap.  These  rooms  are  decorated  with 
stalactites  suspended  from  the  roof.  They  are  exceed- 
ingly picturesque. 

On  and  about  the  dam  are  numerous  siliceous  cores 
of  concentric  layers  of  silica.  They  are  from  one-half 
inch  to  several  inches  in  diameter  and  from  an  inch 
to  several  feet  in  length.  The  waters,  which  formerly 
came  up  through  the  center  of  the  cores,  have  kept 
depositing  their  silica  until  the  vents  were  entirely 
closed,  thus  forming  the  siliceous  core. 

In  the  American  Journal  of  Science,  3d  series,  vol- 
ume 7,  1889,  page  351,  Mr.  W.  H.  Weed,  who  has 
studied  the  formation  of  sinters  in  the  Yellowstone 
Park,  states  that  the  deposit  may  be  due,  either  to  relief 
of  pressure,  to  cooling,  to  chemical  reactions  between 
different  waters,' to  simple  evaporation,  or  to  the  action 
of  algae.  In  the  last  case  the  silica  forms  a  gelatinous 
layer  upon  the  algous  growths,  and  this,  after  the  death 
of  the  algae,  gradually  hardens  to  sinter.  While  all 
of  the  above  actions  have  taken  place  on  different  parts 
of  the  dam,  the  actions  which  have  formed  the  silice- 
ous cores  are  the  relief  of  pressure  and  cooling  of  the 


No.  1 ,  1 9 1 3 . )      Kefly  and  A nsjach— Jemez  Plateau  Waters  9 

water.  Since  the  cores  have  formed  under  the  sur- 
face of  the  ground,  their  formation  could  not  be  due  to 
evaporation  or  to  the  action  of  algae,  as  algae  are 
found  only  at  some  distance  from  the  mouth  of  the 
springs  on  the  surface. 

Because  the  waters  from  the  springs  on  the  dams  are 
strongly  alkaline  they  carry  large  amounts  of  silica 
when  under  pressure  and,  as  soon  as  this  pressure  is 
removed,  a  large  amount  of  the  silica  is  deposited, 
forming  the  cores. 

The  waters  of  the  springs  come  to  the  surface  after 
encountering  a  granite  wall  in  their  southern  course, 
which  crosses  the  country  in  an  east  and  west  direc- 
tion ;  hence  the  line  of  springs. 

Reagan  gives  the  geology  of  the  dam  as  follows : 
"These  springs  existed  in  former  geologic  time 
and  then  dammed  the  river  with  their  deposits  the 
same  as  today.  The  remains  of  the  first  dam  is 
nearly  one  thousand  feet  above  the  present  one; 
and,  as  the  river  has  cut  its  channel  down,  a  suc- 
cession of  dams  in  step-like  order  has  been  forme  1. 
These  dams,  therefore,  are  evidence  that  Canon 
San  Diego  was  not  formed  altogether  by  a  fault- 
ing of  the  strata ;  but  that  the  Jemez  river  has  here 
chiseled  out  for  itself  the  present  channel.  They 
also  indicate  that  the  Jemez  plateau  has  been  raised 
by  a  series  of  uplifts,  each  dam  marking  the  period 
of  rest." 

THE  SULPHURS. 

To  the  north  of  Pelado,  about  thirteen  miles  north- 
east of  the  Soda  Dam  and  the  Jemez  Hot  Springs,  on 


10  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

the  very  top  of  the  Jemez  Plateau  are  the  famous  sul- 
phur springs  and  still  further  to  the  northeast  are  the 
San  Antonio  springs.  The  latter  attain  a  temperature 
about  the  same  as  that  of  the  Indian  springs  to  the 
east  of  the  Jemez  river.  The  Sulphur  springs  deposit 
sulphur  in  considerable  quantity  as  the  name  indicates — 
(see  analysis  of  spring  No.  11) — and  their  site  was 
obtained  as  a  mineral  claim.  They  are  owned  by  the 
Otero  family  and  their  value  is  now  estimated  at  $100,- 
000.00. 

Many  years  ago  the  Oteros  erected  a  mill  for  the 
extraction  of  sulphur  from  the  large  sulphur  deposits, 
but  later  heirs  to  the  estate  have  let  the  mill  lie  idle 
for  the  past  fifteen  years  and  today  the  expensive  .ma- 
chinery is  rotting  for  lack  of  attention.  Mr.  Alfredo 
Otero,  the  present  owner,  states  that  the  extraction  of 
sulphur  was  discontinued  because  of  the  excessive 
freight  rates,  and  also  because  of  the  fact  that,  as  the 
diggings  became  deeper,  the  temperature  increased  to 
such  a  point  that  it  was  impossible  for 'a  man  to  work 
in  the  mine. 

What  was  considered  to  be  an  average  sample  of 
the  crude  deposit  in  the  old  tunnel  was  analyzed  quan- 
titatively for  free  sulphur  showing  it  to  contain  about 
75%  free  sulphur. 

FIELD  OPERATIONS. 

The  plateau  was  visited  in  October,  1911,  by  a  party 
of  professors  and  students  of  the  University  of  New 
Mexico.  The  party  included  Mr.  J.  A.  Pynch,  Asso- 
ciate Professor  of  Geology  and  State  Geologist,  Mr. 
J.  D.  Clark,  Associate  Professor  of  Chemistry,  Mr. 


No.  1 ,  1913.)     Ke11y  and  A nsfach—Jen-. ez  Plateau  Waters  \  \ 

A.  O.  Weese,  Assistant  Professor  of  Biology,  and 
several  students  of  the  University,  among  them,  Mr. 
E.  V.  Anspach.  A  very  hasty  examination  of  the 
topography  of  the  district  was  made,  nothing  further 
being  done  at  this  time. 

In  October,  1912.  Professor  Clark  and  Mr.  C.  Kelly 
made  a  more  extended  visit  to  the  district.  During 
this  visit  the  sarr.ples  of  waters,  sinters,  and  gas,  which 
were  used  in  the  analyses,  were  collected,  temperatures 
of  the  waters  of  the  springs  taken,  and  a  close  exam- 
ination of  the  external  appearance  of  the  springs  was 
made.  Note  was  also  made  of  the  clearness  or  turbid- 
ity of  the  waters,  and  the  presence  or  absence  of 
hydrogen  sulphide.  The  test  for  the  latter  was  merel) 
by  sense  of  smell. 

The  operations  of  collecting  and  preparing  the  sam- 
ples for  transportation  were  carried  out  as  simply  as 
possible.  -  The  water  was  bottled  in  glass-stoppered 
bottles,  which  were  then  sealed  with  sealing  wax  or 
paraffin.  In  every  case  care  was  taken  to  clean  the 
receptacle  thoroughly  and  to  rinse,  before  bottling,  with 
some  of  the  water  to  be  examined. 

The  difficulties  in  the  way  of  collecting  and  trans- 
porting large  quantities  of  water  in  a  region  compara- 
tively inaccessible  were  such  that  the  collection  of 
large  samples  of  water  from  any  one  spring  was  im- 
possible. The  size  of  the  sample  was  necessarily  small 
and  varied  from  a  half  liter  to  one  liter. 

The  thermometer  used  in  taking  the  temperatures  of 
the  various  springs  was  a  Centigrade  thermometer 


12  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

which  had  been  carefully  standardized  with  a  standard 
thermometer. 

METHODS  OF  ANALYSIS. 

Because  of  the  limited  time  at  our  disposal  for  ma^c- 
ing  this  study  we  used  the  rapid  methods  of  analysis 
described  below  taken  largely  from  Water  Supply 
Paper  No.  236  of  the  United  States  Geological  Sur- 
vey. The  author  of  the  above  paper  states  that  with 
these  methods  one  can  estimate  tue  principal  acids  and 
bases  with  moderate  accuracy.  We  would  advise  any- 
one making  a  more  thorough  investigation  of  the 
waters  we  have  studied  to  use  the  refined  methods 
described  in  more  technical  works  on  water  analysis. 
Among  such  works  are,  Bulletin  47  of  the  United 
States  Geological  Survey,  and  a  bulletin  of  the  De- 
partment of  the  Interior  entitled,  'Analyses  of  the 
Waters  of  the  Hot  Springs  of  Arkansas,  by  J.  K.  Hay- 
wood,  and  Geological  Sketch  of  Hot  Springs,  Arkan- 
sas, by  Walter  Harvey  Weed." 

In  each  sample  of  water  we  determined : 

Total  dissolved  solids 

Silica 

Ferric  oxide  (Fe2O:{) 

Aluminum  oxide  (A12O;!) 

Calcium 

Magnesium 

Sodium 

Potassium 

Sulphates 

Carbonates 

Bicarbonates 


No.  1.1913.)      Kelly  and  Ansfach- Jemez  Plateau  Waters  \% 

Chlorine 

Nitrates 

Total  acidity 

Total  iron 

Hydrogen  sulphide 

Total  suspended  solids  was  also  determined  in  one 
of  the  waters,  viz.,  that  from  the  Mud  Geyser. 

In  the  samples  of  gas  collected  from  the  Original 
Spring  we  determined : 

Carbon  dioxide 

Methane 

Hydrogen 

Oxygen 

Nitrogen 

In  the  sinters  we  analysed  qualitatively  for  the  fol- 
lowing : 

Arsenic 

Lithium 

Phosphates 

Borates 

In  addition  to  this  we  analysed  quantitatively  for 
s-ulphur  in  the  mud  of  the  Mud  Geyser,  since  it  gave 
evidence  of  containing  an  unusually  large  amount  of 
that  element  in  the  free  state. 

METHODS  OF  ANALYSIS  OF  THE  WATERS. 

TCTAL  DISSOLVED  SOLIDS. 

Total  dissolved  solids  were  regularly  determined  on 
250  cubic  centimeters  of  the  filtered  sample,  which  was 
evaporated  to  dryness  on  the  water  bath  in  a  tared 
platinum  dish,  dried  at  about  180  degrees  for  one  hour. 


14  Bulletin  University  of  New  Mexico      ',Chem.  Ser.,  Vol.  1 

cooled  and  weighed.     The  residue  was  computed  to 
parts  per  million  of  total  dissolved  solids. 

The  determination  of  dissolved  solids  is  usually  re- 
garded as  desirable,  if  for  no  other  reason  than  to 
serve  as  a  control  of  the  summation  of  the  determina- 
tions of  the  individual  constituents;  but  the  complexity 
of  these  waters  and-  the  relations  of  the  combined  salts 
are  such  that  it  is  not  possible  to  arrive  at  the  same 
end  by  the  determination  of  dissolved  solids  and  the 
summation  of  the  individual  constituents.  The  action 
of  free  silica,  which  is  an  abundant  constituent  of  the 
waters,  is  to  set  free  during  the  process  carbonic  acid 
from  the  carbonates  and  boric  acid  from  the  borates ; 
to  magnify  the  tendency  of  the  chlorides  of  calcium, 
magensium,  and  lithium  ;  to  exchange  chlorine  for  oxy- 
gen, and,  if  the  temperatures  be  pushed  sufficiently 
high,  to  dehydrate  the  silica  and  to  volatilize  sulphuric 
acid.  Furthermore,  the  extent  of  such  action  is  varia- 
ble and  indeterminate.  There  is  obvious  reason,  there 
fore,  for  the  difficulty  which  we  experienced  in  obtain- 
ing results  on  the  individual  constituents  whose  sum 
would  equal  the  total  solids  as  determined  above.  In 
nearly  all  the  waters  under  consideration  the  sum  of 
individual  constituents  was  considerably  in  excess  of 
the  total  solids.  This  was  due  in  part  to  the  reasons 
given  above  and  also  to  the  fact  that  the  ferrous  iron, 
as  well  as  the  ferric  iron,  was  calculated  as  ferric  oxide, 
thereby  introducing  oxygen  which  was  not  present  in 
the  total  solids. 

SILICA. 

The  residue  from  the  determination  of  total  dissolved 


No.  1,  1913.)     Kelly  and  Ansfrack— Jemez  Plateau  Waters  \§ 

solids,  after  being  gently  heated  until  the  organic  mat- 
ter was  carbonized  or  wholly  destroyed,  was  moistened 
with  hydrochloric  acid  (1:1)  and  the  dish,  covered 
with  a  watch  glass,  was  heated  on  the  water  bath  for 
a  few  minutes.  After  treatment  with  acid  had  been 
repeated,  if  necessary,  the  sides  of  the  dish  were  thor- 
oughly rubbed  down,  and  the  mass  was  evaporated  to 
dryness.  The  residue  was  again  treated  with  two  or 
three  cubic  centimeters  of  the  acid  and  some  distilled 
water,  \vas  heated  on  the  wrater  bath,  and  was  finally 
separated  from  the  solution  by  filtration  through  ash- 
less  filter  paper.  The  insoluble  part  was  thoroughly 
washed  with  hot  water  containing  hydrochloric  acid, 
ignited  in  a  tared  platinum  crucible,  cooled  and 
weighed.  It  was  moistened  with  a  few  drops  of  sul- 
phuric acid  (specific  gravity  1.84),  and  the  silica  was 
volatilized  with  hydroflouric  acid,  after  which  the  cru- 
cible was  again  ignited,  cooled  and  weighed.  The  part 
volatilized  by  hydrofluoric  acid  was  computed  to  parts 
per  million  of  silica.  The  non-volatile  residue  was  dis- 
solved in  hydrochloric  acid  and  added  to  the  filtrate 
from  the  silica. 

IRON  AND  ALUMINIUM. 

The  iron  in  the  filtrate  from  the  determination  of 
silica  was  oxidized  by  boiling  the  solution  with  a  few 
drops  of  nitric  acid  (specific  gravity  1.42).  After  a 
slight  excess  of  ammonium  hydrate  had  been  added, 
the  liquid  was  heated  for  a  few  minutes  to  precipitate 
the  hydroxides  of  iron  and  aluminium,  which  were  then 
removed  by  filtration  and  washed  with  hot  water  con- 
taining a  little  ammonium  chloride.  The  precipitate 


jy  Bulletin  University  of  New  Mexico     [Chem.  Ser.;  Vol.  1 

was  dried,  placed  iii  a  tared  platinum  crucible,  ignited 
and  weighed  as  combined  oxides  of  iron  and  aluminium. 

TOTAL  IRON. 

In  several  cases  where  the  amount  of  iron  and  alu- 
minium oxides  was  large,  a  determination  of  total  iron 
was  made.  This  was  done  by  fusing  the  oxides  of 
iron  and  aluminium  with  potassium  hydrogen  sulphate, 
and  transferring  the  fused  mass  to  a  beaker  containing 
sodium  hydrate  in  solution,  which  precipitated  the  iron 
as  ferric  hydrate  and  retained  the  aluminium  in  solu- 
tion as  sodium  aluminate.  The  precipitate  was  sepa- 
rated from  the  liquid  by  filtration,  washed,  dried,  trans- 
ferred to  a  tared  platinum  crucible,  ignited  and 
weighed  as  ferric  oxide.  From  the  weight  of  ferric 
oxide  the  amount  of  iron  \vas  calculated. 
CALCIUM. 

The  filtrate  from  the  determination  of  iron  and 
aluminium  was  diluted  to  a  definte  volume,  usually  100 
cubic  centimeters,  and  was  divided  into  two  equal 
parts.  One  part  was  used  for  the  determination  of 
calcium  and  magnesium  and  the  other  part  for  the 
determination  of  sulphates  and  alkalies.  After  the 
portion  for  the  determination  of  calcium  and  mag- 
nesium had  been  heated  to  boiling  in  a  beaker,  it  was 
made  slightly  alkaline  with  ammonium  hydrate ;  am- 
monium oxalate  in  the  form  of  hot  five  per  cent  aqueous 
solution  was  then  added  to  it  in  sufficient  amount  to 
convert  all  the  calcium  and  magnesium  into  oxalates. 
Ten  cubic  centimeters  were  usually  added,  but  more 
was  used  if  the  figure  for  total  solids  indicated  that 
this  amount  was  not  enough.  The  mixture  was  di- 


No.  1,  1913.)      Kelly  and  Ans^acK—Jemez  Plateau  Waters  17 

gested  not  less  than  three  hours  in  order  to  precipitate 
all  the  calcium  and  to  dissolve  the  magnesium  oxalate. 
The  solution  was  filtered  and  the  precipitate  washed 
with  hot  water  containing  a  little  ammonia,  no  special 
care  being  taken  to  transfer  all  the  calcium  oxalate 
from  the  flask  to  the  funnel.  The  flask  in  which  the 
precipitation  was  made  was  then  placed  under  the 
funnel,  and  while  the  precipitate  was  agitated  by  a 
stream  of  hot  water  from  a  wash  bottle,  dilute  sul- 
phuric acid  (1  to  3 )  was  poured  on  till  the  precipitate 
was  completely  decomposed  and  dissolved,  after  which 
the  filter  paper  was  thoroughly  washed  with  hot  water. 
If  this  operation  is  skillfully  performed,  the  calcium 
precipitate  is  easily  dissolved  and  twenty  cubic  centi- 
meters of  the  dilute  acid  is  amply  sufficient  for  the 
purpose.  The  solution  of  calcium  was  diluted  to  about 
one  hundred  cubic  centimeters  with  hot  distilled  water, 
brought  to  boiling,  and  titrated  with  N/20  potassium 
permanganate. 

MAGNESIUM. 

The  filtrate  from  the  calcium,  having  been  made 
slightly  acid  with  hydrochloric  acid,  was  concentrated 
till  the  salts  began  to  crystallize.  An  excess  of  a  ten 
per  cent  solution  of  sodium  ammonium  phosphate  was 
added,  and  the  liquid  was  allowed  to  cool.  Finally  it 
was  made  distinctly  alkaline  with  ammonium  hydrate 
and  set  aside  not  less  than  six  hours  in  order  to  insure 
complete  precipitation  of  the  magnesium.  Two  cubic 
centimeters  of  strong  ammonia  (specific  gravity  0.90) 
was  usually  sufficient  in  a  volume  of  fifty  to  seventy- 
five  cubic  centimeters.  A  large  excess  of  ammonia  is 


18  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

distinctly  disadvantageous.  The  precipitate  was  sepa- 
rated by  filtration  and  was  washed  by  decantation  with 
water  containing  a  little  ammonia,  till  the  excess  of 
precipitant  was  removed.  The  precipitate  in  the  beaker 
and  on  the  paper  was  dissolved  in  five  cubic  centi- 
meters of  five  per  cent  acetic  acid  and  about  forty 
cubic  centimeters  of  hot  water.  Five  cubic  centimeters 
of  a  five  per  cent  ammonium  acetate  solution  was 
added  and  the  solution  was  titrated  with  standard 
uranium  solution,  care  being  taken  to  boil  the  solution 
vigorously  before  noting  the  final  end  point,  which  is 
found  by  adding  a  drop  of  the  liquid  to  a  drop  of  half- 
saturated  solution  of  potassium  ferro-cyanide  on  a 
white  porcelain  plate. 

It  is  important  to  have  a  constant  amount  of  solu- 
tion, as  the  end  point  varies  somewhat  with  the  vol- 
ume. The  quantity  of  phosphate  that  is  titrated  should 
be  such  that  ore  to  twenty  cubic  centimeters  of  ura- 
nium solution  may  be  added. 

SULPHATE  RADICLE. 

The  usual  gravimetric  method  was  employed  for  the 
determination  of  sulphates.  One-half  the  filtrate  from 
the  determination  of  iron  was  slightly  acidulated  with 
hydrochloric  acid  and  was  heated  nearly  to  boiling. 
Excess  of  barium  chloride  in  hot  ten  per  cent  solution 
was  then  added,  after  which  the  liquid  was  digested  on 
the  hot  plate  for  at  least  thirty  minutes.  The  precipi- 
tate of  barium  sulphate  was  removed  by  filtration, 
thoroughly  washed  with  hot  water,  dried,  ignited  am! 
weighed.  The  amount  of  sulphates  as  parts  per  mil- 
lion of  SO4  was  computed  from  that  weight. 


No,  1,  1913.)       Kelly  and  Ansfach  — Jemez  Plateau  Waters  JQ 

SODIUM    AND    POTASSIUM. 

The  filtrate  from  the  sulphate  determination  was 
treated  with  ammonia  and  ammonium  carbonate  and 
was  filtered.  The  filtrate  was  evaporated  to  dryness 
on  the  water  bath,  heated  to  expel  ammonium  salts. 
and  digested  with  a  few  cubic  centimeters  of  distilled 
water.  The  filtrate  from  this  operation  was  heated, 
and  barium  and  calcium  were  precipitated  with  am- 
monium carbonate  and  were  removed  by  filtration, 
after  which  the  filtrate  was  evaporated  to  dryness  and 
heated  to  expel  ammonium  salts.  The  residue  was  di- 
gested with  four  or  five  cubic  centimeters  of  water, 
warmed,  and  treated  again  with  ammonia  and  am- 
monium carbonate  to  remove  traces  of  barium  and 
calcium.  The  solution  was  then  filtered  into  a  small 
porcelain  dish  and  evaporated  to  dryness.  The  resi- 
due was  heated  neirly  to  fusion  and  weighed.  The 
alkaline  chlorides  in  the  dish  were  dissolved  in  a  little 
water  and  were  filtered  through  an  ashless  filter  paper, 
which  was  then  washed,  ignited  in  the  porcelain  dish, 
and  weighed.  The  difference  in  weights  was  calcu- 
lated as  sodium  and  potassium  chlorides.  The  filtrate 
was  evaporated  to  dryness  and  treated  with  eighty  per 
cent  alcohol,  and  platinic  chloride.  The  precipitate  of 
potassium  platinic  chloride  was  removed  by  filtration, 
washed  with  eighty  per  cent  alcohol,  and  dissolved  on 
the  filter  with  warm  water.  The  solution  was  evapor- 
ated to  dryness  in  a  tared  platinum  or  porcelain  dish 
and  weighed  as  potassium  platinic  chloride.  From  the 
weight  of  the  potassium  double  salt  the  parts  per 
million  of  potassium  were  computed. 


'20  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

CARBONATE    AND    BICARBONATE    RADICLES. 

Estimates  of  the  carbonate  and  bicarbonate  radicles 
were  made  on  the  same  fifty  cubic  centimeter  sample 
of  the  water,  which  was  filtered  if  necessary.  Ten 
drops  of  pler.olphthalein  were  added  to  the  measured 
sample  in  a  porcelain  dish  of  convenient  size  and  the 
sample  was  titrated  with  N/50  potassium  acid  sul- 
phate solution.  The  number  of  cubic  centimeters  of 
acid  used,  "multiplied  by  24,  equals  parts  per  million  of 
the  carbonate  radicle.  Two  drops  of  methyl  orange- 
were  added  to  the  same  liquid  and  the  titration  was 
continued.  The  total  amount  of  acid  used,  minus  twice 
that  required  for  the  first  end  point  equals  that  equiva- 
lent to  the  bicarbonate  present.  The  latter  figure,  ex- 
pressed in  cubic  centimeters  and  multiplied  by  24. -1 
equals  parts  per  million  of  the  bicarbonate  radicle. 

CHLORINE. 

The  usual  volumetric  procedure  was  employed  for 
the  determination  of  chlorine.  One  hundred  cubic 
centimeters  of  the  sample  were  placed  in  a  porcelain 
dish,  one  cubic  centimeter  of  a  five  per  cent  potassium 
chromate  solution  was  added  and  standard  silver  ni- 
trate then  added  from  a  burette,  till  the  first  faint 
reddish  tint  appeared.  The  chlorine  in  parts  per  mil- 
lion was  then  computed. 

In  the  acid  waters  it  was  necessary  to  neutralize  with 
bicarbonate  of  soda  before  adding  the  potassium  chro- 
mate, because  the  sulphuric  acid  of  the  water  would 
form  chromic  acid  with  the  chromate,  thereby  darken- 
ing the  solution  so  much  as  to  obliterate  the  end  point 
of  the  determination, 


Xo.  1,  1913.)      fafly  and  Ansfrach—Jemez  Plateau  Waters  21 

NITRATES. 

The  phenolsnphonic  acid  method  was  used  for  the 
determination  of  nitrates.  Fifty  cubic  centimeters  of 
the  clear  water  was  evaporated  to  dryness  in  a  porce- 
lain dish  on  a  water  bath  with  a  few  drops  of  sodium 
carbonate  solution.  One  cubic  centimeter  of  phenol- 
sulphonic  acid  was  quickly  and  thoroughly  rubbed  over 
the  residue  in  the  dish,  after  which  ten  cubic  centi- 
meters of  distilled  water  were  added  and  the  solution 
was  stirred  till  it  was  thoroughly  mixed.  After 
enough  ammonium  hydrate  to  render  the  liquid  alka- 
line had  been  added,  the  solution  was  transferred  to  a 
Xessler  tube  and  was  diluted  to  the  mark- with  distilled 
water.  The  yellow  color  developed  by  the  nitrates  was 
compared  with  similar  shades  in  Nessler  tubes  con- 
taining solutions  of  known  amounts  of  potassium  ni- 
trate that  had  been  treated  with  phenolsulphonic  acid 
and  ammonia.  The  results  are  reported  as  parts  per 
million  of  the  nitrate  radicle. 

Though  this  procedure  is  comparatively  accurate  for 
estimating  the  amount  of  nitrogen  actually  present  as 
nitrates  at  the  time  of  the  test,  it  must  be  emphatically- 
stated  that  the  reported  nitrate  figures  do  not  repre- 
sent the  amount  of  nitrogen  present  as  nitrates  in  .the 
waters  when  the  samples  were  collected.  Practical 
considerations  made  it  impossible  to  perform  the  test 
until  considerable  time  had  elapsed  after  the  samples 
had  been  collected,  and  though  the  value  of  the  deter- 
mination a§  an  index  of  the  condition  of  the  waters 
at  the  time  the  samples  were  taken  is  probably  not 
great,  the  amounts  found  may  furnish  some  in  forma- 


22  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

tion  regarding  the  amount  of  organic  matter  that  is 
present,  and  this  feature  is  the  excuse  for  the  presenta- 
tion of  the  nitrate  figures  in  the  analytical  data. 

TOTAL    ACIDITY. 

If  the  water  under  examination  contained  free  min- 
eral acid  a  convenient  amount  of  the  sample,  filtered  if 
necessary,  was  titrated  with  X/10  sodium  carbonate  in 
the  presence  of  methyl  orange  indicator.  If  fifty 
cubic  centimeters  of  the  water  is  titrated,  the  number 
of  cubic  centimeters  of  N/10  alkali  used,  multiplied  by 
98,  gives  the  result  in  parts  per  million  of  free  sul- 
phuric acid. 

HYDROGEN    SULPHIDE. 

A  measured  quantity,  say  ten  cubic  centimeters,  of 
N/10  arsenious  acid  solution  was  put  into  a  300  c.  c. 
Hask,  and  twenty  cubic  centimeters  of  the  water  added, 
well  mixed,  and  sufficient  hydrochloric  acid  added  to 
produce  a  distinct  acid  reaction;  this  produces  a  pre- 
cipitate of  arsenic  sulphide,  and  the  liquid  itself  is 
colorless.  The  whole  is  then  diluted  to  300  cubic  cen- 
timeters, filtered  through  a  dry  filter  into  a  dry  vessel, 
100  cubic  centimeters  of  the  filtrate  taken  out  and  neu- 
tralized with  sodium  carbonate,  then  titrated  with 
N/10  iodine  and  starch.  The  quantity  of  arsenious 
acid  so  found  is  deducted  from  the  original  ten  cubic 
centimeters  and  the  remainder  multiplied  by  the  req- 
uisite factor  for 'hydrogen  sulphide,  which  is  reported 
as  parts  per  million. 

ANALYSIS  OF  THE  SIXTKRS, 
The  analysis  of  the  sinters  was  merely  a  qualitative 


No.  1,  1913.)     KeTJy  and  Ans^ach—Jemez  Plateau  Waters  23 

test  for  substances  that  would  probably  be  present  in 
too  small  quantity  to  be  discovered  in  the  small 
amounts  of  water  which  we  were  forced  to  use  in  the 
analysis. 

Arsenic  was  tested  for  by  means  of  the  Marsh  Ap- 
paratus, phosphates  by  the  regular  molybdate  method 
of  qualitative  analysis,  and  lithium  and  boron  tested 
for  by  means  of  an  Adam  Hilger  best  grade  wave- 
length spectroscope. 

ANALYSIS  OF  THE  GAS. 

The  analysis  of  the  gas  collected  from  the  "Original 
Spring,"  was  made  according  to  the  methods  given  in 
Hempel's  "Gas  Analysis''. 

The  carbon  dioxide  was  absorbed  by  means  of  a 
potassium  hydroxide  solution.  Oxygen  was  absorbed 
by  means  of  sticks  of  yellow  phosphorous.  Air  was 
then  added  to  the  remaining  mixture  of  gases  and  the 
hydrogen  was  taken  out  by  passing  the  mixture  over 
heated  palladinized  asbestos,  thus  converting  the  hydro- 
gen present  into  water.  Methane  was  determined  by 
exploding  an  aliquot  portion  of  the  gas  and  absorbing 
the  carbon  dioxide  formed  by  passing  it  into  potas- 
sium hydroxide  solution.  After  the  removal  of  the 
above  constituents,  the  remainder  of  the  gas  present 
was  assumed  to  be  nitrogen. 

The  gas  from  this  "spring  seemed  to  be  a  fair  average 
of  the  gases  evolved  from  the  springs  of  the  Jemez 
Hot  Springs  group  and  for  this  reason  this  gas  was 
taken  for  the  analysis.  Although  we  wrere  unable  to 
detect  any  hydrogen  sulphide  in  the  gas  by  the  sense  of 


24  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

smell,  a  small  amount  was  undoubtedly  present  as 
shown  by  the  fact  that  the  white  lead  paint  on  the  base 
of  the  summer  house  over  the  spring  had  been  entirely 
blackened  by  the  action  of  hydrogen  sulphide.  How- 
ever, we  did  not  analyse  the  gas  for  hydrogen  sulphide 
content. 

SULPHUR  DETERMINATION  IN  MUD  OF 
MUD  GEYSER. 

Because  the  mud  in  the  Mud  Geyser  showed  evi- 
dence of  having  a  high  free  sulphur  content,  a  quanti- 
tative determination  of  that  element  was  made  on  the 
mud. 

The  mud  was  thoroughly  dried  and  a  weighed  por- 
tion was  put  in  an  extraction  shell,  which  was  in  turn 
placed  in  a  Soxhlet  extractor  and  the  sulphur  extracted 
by  carbon  disulphide.  The  carbon  disulphide  was  then 
evaporated  and  the  residue  weighed  as  pure  sulphur. 

As  a  rough  check  on  the  above  determination  and 
also  to  determine  the  amount  of  sulphur  present  in  the 
form  of  insoluble  sulphides,  another  weighed  portion 
of  the  dried  mud  was  placed  on  a  filter  and  washed  with 
hot  water  until  free  from  soluble  sulphides  and  sul- 
phates. The  residue  on  the  filter  was  then  washed 
into  a  flask,  about  100  cubic  centimeters  of  nitric  acid 
added,  and  the  mixture  boiled  until  the  evolution  of 
nitrogen  peroxide  fumes  was  faint-.  It  was  then  filtered 
and  the  filtrate  heated  almost  to  boiling.  A  hot  aque 
ous  solution  of  barium  chloride  was  then  added  and 
the  mixture  digested  on  the  hot  plate  for  half  an  hour. 
The  precipitate  of  barium  sulphate  was  then  filtered  off. 


No.  1.  1913.)     Kelly  and  Ansfrach— Jemez  Plateau  Waters  25 

washed  with  hot  water,  ignited  and  weighed.  The  per- 
centage of  sulphur  was  then  calculated  from  this 
weight. 

DESCRIPTION  AXD  LOCATION  OF  THE 
SPRINGS. 

Spring  No.  1.  This  is  the  so-called  Soda  Spring  at 
Jemez  Hot  Springs,  New  Mexico.  The  vent,  which 
lies  about  the  center  of  the  town,  is  in  the  river  bottom, 
the  waters  coming  up  through  the  river-bed  gravels.  A 
green  scum  of  organic  matter  fringes  the  vent  and  a 
deposit  of  the  color  of  ferric  hydroxide  lines  it  inside. 
The  pool  is  about  one  foot  in  diameter.  A  considerable 
quantity  of  gas  is  being  evolved.  Several  larval  worms 
about,  three  inches  long  are  in  the  water  just  outside 
the  pool. 

Spring  No.  2.  This  spring  is  known  as  the  Original 
Spring.  It  lies  about  thirty  yards  northeast  of  the 
Soda  Spring.  The  pool,  into  which  the  spring  flows, 
is  about  seven  feet  in  diameter  and  three  feet  deep.  It 
is  lined  with  a  deposit  of  the  color  of  ferric  hydroxide 
and  a  green  scum  of  organic  matter  fringes  it  at  the 
surface  of  the  water.  A  large  quantity  of  gas  bubbles 
from  the  spring.  The  pool  is  covered  by  a  small  sum- 
mer house  and  pipes  lead  some  of  the  water  to  the  bath 
house  about  fifty  feet  to  the  south. 

Spring  No.  3.  This  is  the  Iron  Spring,  so-called  be- 
cause of  the  color  of  the  deposit,  this  color  being  that  of 
iron  rust.  The  color  is  not  due  to  iron  oxide  but  is  due 
to  a  red  algous  growth.  The  spring  is  situated  about 
fifty  feet  southeast  of  the  So'da  Spring.  The  deposit 


2(5  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

does  not  form  a  sinter  but  remains  soft  and  flaky.  The 
banks  of  the  small  stream  flowing  from  the  spring  are 
covered  with  a  dark  green  deposit  of  organic  matter 
at  the  edge  of  the  water.  A  platform  is  built  over  the 
spring  with  a  cement  box  in  the  center  into  which  -the 
spring  flows. 

Spring  No.  6.  This  spring  lies  on  top  of  and  to  the 
extreme  west  end  of  the  Soda  Dam.  The  pool  of  the 
spring  is  about  one  and  one-half  feet  long  by  one  foot 
wide  and  six  inches  deep.  The  water  is  strongly 
charged  with  gas  having  a  faint  odor  of  hydrogen  sul- 
phide. The  bottom  of  the  pool  is  covered  with  a  dark 
green  lining  of  organic  matter. 

Spring  No.  8.  The  spring  bubbles  up  through  nu- 
merous vents  into  a  submerged  bottomless  bath-tub  in 
the  Main  Bath  House  at  Sulphur  Springs,  New  Mex- 
ico, about  fifteen  miles  north  of  Jemez  Hot  Springs. 
The  water,  which  is  very  turbid,  deposits  mud  in  the 
bottom  of  the  tub,  and  the  gas  from  the  spring,  which 
has  a  strong  odor  of  hydrogen  sulphide,  deposits  sul- 
phur crystals  on  the  sides  of  the  bath-tub  and  walls  of 
the  house. 

Spring  No.  9.  This  is  known  as  the  Sour  Spring. 
It  lies  a  short  distance  to  the  north  of  the  Main  Bath 
House  at  Sulphur  Springs.  The  water  tastes  strongly 
of  sulphuric  acid.  The  pool  over  the  vent  is  about  n 
foot  square  and  one  foot  deep.  A  small  amount  of  gas 
accompanies  the  water.  Solfataras  within  twenty  feet 
and  to  the  south  of  the  spring  are  blowing  steam  and 
gas,  which  has  a  temperature  of  eighty-nine  degrees 
Centigrade,  or  about  two  degrees  less  than  the  boiling 


No.  1.  1913.)     Kelly  and  Ansfrach— Jemez  Plateau  Waters  27 

point  of  water  at  this  altitude.  Within  twenty-five  feet 
of  the  Sour  Spring  are  vents,  said  to  be  the  openings 
of  an  extinct  geyser.  Pine  logs  near  the  spring  are 
badly  charred  by  the  sulphuric  acid  in  the  water. 

Spring  Xo.  10.  The  Alum  Spring,  as  it  is  called, 
lias  a  taste  of  strong  alum  water.  It  lies  in  the  bed  of 
an  arroyo  about  three  hundred  feet  to  the  east  of  the 
Sour  Spring.  The  pool  is  about  the  same  size  as  that 
of  the  Sour  Spring,  but  the  vents  are  much  larger, 
being  three  inches  in  diameter.  A  large  amount  of  gas 
comes  up  throv.gh  the  water  in  the  pool  and  also 
through  the  sand  in  the  bed  of  an  arroyo  around  the 
spring. 

Spring  Xo.  11.  The  Mud  Geyser  would  hardly  be 
called  a  spring  because  no  water  flows  out  of  it.  This 
geyser  lies  almost  due  north  of  the  Alum  Spring.  The 
pool  of  the  geyser,  which  is  about  seven  feet  in  diame- 
ter and  three  feet  deep,  seems  to  maintain  a  constant 
level  of  water,  except  when  an  excess  of  rain-water 
causes  it  to  overflow.  Even  the  hot,  dry  days  of  sum* 
mer  do  not  evaporate  the  water  sufficiently  to  make, 
much  of  a  change  in  the  level  of  the  water.  An  ex- 
ceedingly large  amount  of  gas  comes  up  through  the 
water  from  a  great  many  vents  in  the  bottom  of  the 
pool.  The  odor  of  hydrogen  sulphide  is  very  strong. 
The  escaping  gas  strongly  agitates  the  surface  of  the 
water,  giving  it  the  appearance  of  a  large  vessel  of  vio- 
lently boiling  water.  The  water,  or  mud  as  it  may  be 
called,  has  a  total  of  94,500  parts  per  million  of  sus- 
pended solids.  (See  analysis  of  sinter  No.  11.) 

Spring  Xo.  12.     This  quiet  little  spring,  known  as 


2#  Bulletin  University  of  New  Mexico     CChem.  Ser.,  Vol.  1 

the  Seltzer  Spring,  bubbles  up  into  a  submerged  barrel 
about  two  hundred  yards  up  the  arroyo  from  the  Mud 
Geyser.  The  water  resembles  seltzer  water,  both  in 
its  taste  and  in  its  effect  on  the  human  system.  A  small 
quantity  of  gas,  having  a  very  faint  odor  of  hydrogen 
sulphide,  comes  to  the  surface.  This  gas  has  deposited 
a  small  amount  of  sulphur  on  the  rocks  surrounding 
and  above  the  barrel. 

Spring  No.  13.  This  spring  is  called  the  Electric 
Spring  because  of  the  fact,  residents  say,  that  the  bub- 
bles of  gas  in  it  give  a  sharp  pain,  resembling  a  shock 
from  an  electric  current,  to  an  open  sore  or  fresh  cut 
in  the  flesh.  This  spring  flows  into  a  large  bath-tub 
twelve  feet  long,  four  feet  wide  and  three  feet  deep, 
made  of  logs,  which  are  charred  by  the  highly  acid 
waters  of  the  spring.  The  deposit  of  the  spring  is  very 
light  and  flocculent  and  of  a  light,  yellow  color.  The 
vents  are  very  minute,  but  are  numerous  enough  to 
cause  a  small  stream 'of  water  to  flow  from  the  tub. 
The  spring  is  situated  about  fifty  yards  south  of  the 
Otero  Sulphur  Mill. 

Spring  No.  14.  The  water  comes  from  numerous 
vents  inside  of  a  submerged  bottomless  wooden  bath- 
tub iii  the  Ladies'  Bath  House  at  Sulphur  Springs. 
Mud  settles  from  the  water  and  sulphur  crystals  form 
on  the  sides  of  the  tub.  A  large  amount  of  gas  accom- 
panies the  water  and  gives  a  strong  odor  of  hydrogen 
sulphide. 

Samples  of  the  sinters  numbers  I,  2,  6  and  8  were 
tal  en  from  the  deposits  formed  around  the  edges  of 
the  pools  of  the  springs  of  the  corresponding  numbers ; 


No.  1,1913.;     Kielly  and  Ansjiach  —  Jemez  Plateau  Waters  29 

samples  numbers  11,  13  and  14  were  samples  of  the 
mud  deposited  in  the  bottom  of  the  pools  from  the 
springs  corresponding  to  the  same  numbers ;  the  other 
three  samples  were  taken  as  follows : 

Sinter  Xo.  4.  Sample  taken  from  a  deposit  formed 
around  a  spring  of  multiple  vents  in  the  bed  of  the 
river  at  a  distance  of  about  one  hundred  feet  below  the 
Soda  Dam.  The  mound  on  which  the  springs  occur, 
is  completely  surrounded  by  the  flowing  water  of  the 
river.  One  of  the  vents  throws  a  stream  of  water  at 
an  angle  of  approximately  thirty  degrees  with  the 
horizontal  for  a  distance  of  about  six  feet. 

Sinter  Xo.  5.  This  sample  was  taken  from  the  de- 
posit around  a  small  pool  of  water  along  the  crack  in 
the  middle  of  the  top  of  the  Soda  Dam.  Light  green 
organic  matter  lines  the  pool. 

Sinter  Xo.  7.  This  was  taken  from  around  the  pool 
of  the  spring  at  the  extreme  east  end  of  the  dam. 
This  spring  is  at  present  forming,  by  its  deposits,  a 
large  dome  of  the  dam  directly  over  the  river.  The 
bottom  of  the  pool  of  the  spring  is  coated  with  very 
dark  green  organic  matter. 


1JQ  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

TABLE  OF  TEMPERATURES  OF  THE   SPRINGS. 


Number 

Dat 

e 

Degrees 
Centi- 
grade 

Degrees 
Fahren- 
heit 

1  

Oct.  11, 

1912 

68.5 

155.3 

2   

Oct    11 

1912 

68.0 

154  5 

3    

Oct    11 

1912 

48.8 

1198 

4  

Oct.  11, 

1912 

46.5 

115.7 

5  
6  "... 

Oct.  11, 
Oct.  11, 

1912 
1912 

23.0 
40.0 

73.6 
1040 

7  
8  

Oct.  11, 
Oct.  11, 

1912 
1912 

43.5 
68.5 

110.3 
155.3 

8  
9  

Oct.  12, 
Oct.  12, 

1912 
1912 

41.0 
44.0 

105.8 
112.2 

10  

Oct.  12, 

1912 

15.2 

59.4 

11  
11 

Oct.  12, 
Oct    12 

1912 
1912 

38.0 
31  0 

100.4 
878 

12  

13 

Oct.  12, 
Oct    12 

1912 
1912 

10.4 
37  1 

50.7 
988 

14   . 

Oct    12 

1912 

750 

1670 

14  

Oct.  12. 

1912 

•  70.0 

158.0 

\Yhere  two  temperatures  are  shown  for  one 'spring, 
the  first  temperature  is  that  found  in  the  mud  in  the 
bottom  of  the  pool,  and  the  second  that  found  in  the 
water  of  the  pool. 


No.  1,  1913.)     Kelly  and  Ans£ach—Jemez  Plateau  Waters 


31 


ANALYSIS  OF  THE  WATER  OF  SPRING  No.  1, 

SODA  SPRING,  JEMEZ  SPRINGS,  N.  M. 

Analysed  by  Prof.  J.  D.  Clark. 


Constituents 

Parts  pei- 
Million 

Per  cent  of 
total  material 
in  solution 

SiO, 

82.8 

3.79 

Fe.O,    I 
A12"03    J  

6.0 

.27 

Ca    

136.8 

6.25 

6.1 

.28 

Xa    

538.6 

24.63 

K    

71.9 

3.24 

SO4    

61.6 

2.82 

co::  

0.0 

0.00 

HC03    

503.6 

23.07 

Cl    

779.8 

35.65 

NO- 

0.0 

0.00 

Acidity  ..  .  .'  

0.0 

0.00 

H2S    

Trace 

Total  Solids, 
heated  one 
hour  at  180°C. 


2187.2 


100.00 


The  qualitative  analysis,  of  the  sinter  from  around 
the  spring  showed  the  following  to  be  present : 

Arsenic  Lithium  Phosphates 

and  also  showed  the  absence  of  borates. 


32 


Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 


ANALYSIS  OF  THE  WATER  OF  SPRING  No.  2. 

ORIGINAL  SPRING,  JEMEZ  SPRINGS,  N.  M. 

Analysed  by  Mr.  E.  V.  Anspach. 


Constituents 


Total  Solids, 
heated  one 
hour  at  180°C.. 


2262:5 


2131.6 


Per  cent  of 
Parts  per          total  material 
Million  in  solution 


Si02  

,.               88.0 

3.89 

Fe203   1 
A1203   j 

14.0 

.61 

Ca    

124.0 

5.48 

Mg  

10.1 

.44 

Na   

408.2 

18.08 

K   

62.6 

2.76 

SO4    

54.4 

2.40 

CO,   

O-.O 

0.00 

HC03  

705.2 

31.16 

Cl    

796.0 

35.18 

N03   

0.0 

0.00 

Acidity  

0.0 

0.00 

H2S    

Trace 

100.00 


The  qualitative  analysis  of  the  sinter  from  around 
the  pool  of  the  spring  showed  the  presence  of  Arsenic, 
Lithium,  and  the  phosphate  radicle,  and  also  showed 
the  absence  of  borates. 


No.  1,  1913.)     Kelly  and  Ansfach— Jemez  Plateau  Waters  33 

The  analysis  of  the  gas  gave  the  following  results : 
Carbon   Dioxide  91.0% 

Oxygen  .  6 

Hydrogen  .  8 

Methane  2 . 4 

Nitrogen  (Remainder)  5.2 

100.0 


34  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

ANALYSIS  01-  THE  WATER  OF  SPRING  No.  3, 

IRON  SPRING,  JEMEZ  SPRINGS,  N.  M. 

Analysed  by  Mr.  Clyde  Kelly. 


Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO2  

105.2 

4.47 

Fe203   I 

4.8 

.20 

Al,03   J 
Ca    

152.0 

6  45 

Mg- 

5  8 

25 

Na 

578  9 

24  59 

K 

68  6 

2  91 

SO, 

70  4 

2  99 

CO, 

0  0 

0  00 

HC03    
Cl    
NO, 

500.2 
868.7 
Trace 

21.25 
36.89 
0  00 

Acidity 

0  0 

0  00 

H2S   .. 

Trace 

0  00 

Total  Solids, 
heated  one 
hour  nt  180°C.  . 

2354.6 
2327.6 

100.00 

No  sinter  was  formed  around  this  spring. 


JN'o.  1,  1913.)     Kelly  and  Ansjach—Jemez  Plateau  Waters 


35 


ANALYSIS  OF  THE:  WATER  FROM  SPRING  No.  6, 

SPRING  ON  WEST  END  OF  THE  SODA  DAM. 

Analysed  by  Mr.  Clyde  Kelly. 


Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO,    
Fe203    { 
A1203    j 
Ca 

58.0 
105.2 
292  8 

1.21 
2.20 
6  12 

Mff  . 

0.3 

0.01 

Na    . 

1069.9 

22.38 

K    

98.5 

2.06 

SO, 

56.6 

1.18 

CO,   . 

0.0 

0.00 

HCO3    

1556.7 

32.56 

Cl    
NO,   . 

1543.4 
Trace 

32.28 
0.00 

Acidity   

0.0 

0.00 

HoS    

Trace 

0.00 

Total  Solids, 
heated  one 
hour  at  180°C.. 


4781.4 


4085.6* 


100.00 


The  analysis  of  the  sinter  from  around  this  spring 
showed  the  presence  of  arsenic,  lithium  and  the  phos- 
phate radicle,  and  the  absence  of  borates. 


36 


BuVetin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 


ANALYSIS  OF  THE  WATER  FROM  SPRING  No.  8, 

MAIN  BATH  HOUSE,  SULPHUR  SPRINGS,  N.  M. 

Analysed  by  Mr.  E.  V.  Anspach. 


Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO.,   

264.0 

9.28 

Fe203    1 
A1203   J 

294.8 

10.36 

Ca    

128  8 

4  52 

Mg  

3.9 

0.14 

Na   

376  8 

13  24 

K 

48  0 

1  69 

S04    

1468.8 

51.61 

CO3    .  .    . 

0  0 

0  00 

HC03    

0.0 

0.00 

Cl    

210  0 

7  37 

NO.{   

0  0 

0  00 

Acidity 

254  8 

H,S   . 

51  1 

1     7Q 

Fe 

10  0 

*2846.2 

100.00 

Total  Solids, 

heated   one 

• 

hour  at  180°C.. 

2849.6 

*    Acidity  and  total  iron  not  included  in  total. 

Qualitative    tests    on  the    mud    from    this    spring 

showed  arsenic,  lithium,  and  the  phosphate  and  borate 
radicles  to  be  absent. 


No.  1,  191  a. )     Kelly  and  Ansfach—Jemez  Plateau  Waters  ; 

ANALYSIS  OF  THE  WATER  FROM  SPRING  No.  9. 

SOUR  SPRING,  SULPHUR  SPRINGS,  N.  M. 

Analysed  by  Mr.  Clyde  Kelly. 


Per  cent  of 

Constituents 

Parts  per 
Million 

total  material 
in  solution 

SiO2  
Fe203   1 

227.6 
172.0 

10.21 
7.72 

Ca    

174.4 

7.83 

Mg 

8.7 

0.39 

Na  
K   
S04    
CO, 

44.7 
12.2 
1574.9 
0  0 

2.01 

o.'ss 

70.68 
0  00 

HCO,    • 
Cl 

0.0 
12  1 

0.00 
0  54 

NO, 

1  5 

0  07 

Acidity  
HoS 

627.2 
Trace 

0  00 

Total  Solids, 
heated  one 
hour  at  180°C.  . 

*2228.1 
2218.8 

100.00 

*    Acidity  not  included  in  total. 

No  sinter  was  formed  around  this  spring. 


Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 


ANALYSIS  OF  THE  WATER  FROM  SPRING  No.  10. 

THE  ALUM  SPRING,  SULPHUR  SPRINGS,  N.  M. 

Analysed  by  Mr.  E.  V.  Anspach. 


Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO2  . 

123.2 

2.48 

Fe203   1 

931.2 

18.71 

A1203    J 
Ca  

354  0 

7  11 

Me- 

9.6 

0  19 

Na    

580  0 

11  65 

K   

134.0 

2.69 

SO4 

2837  2 

56  99 

CO, 

0  0 

0  00 

HC03    
Cl    

0.0 
8  1 

0.00 
0  16 

NO,  . 

1  0 

0  0? 

Acidity  

627  2 

H2S    
Fe    

Trace 
212.8 

Total  Solids, 
heated  one 
hour  at  180°C.  . 

*4978.3 

5252.8 

100.00 

*    Acidity  and  total  iron  not  included  in  total. 

No  sinter  around  this  spring  and  no  deposit  formed, 
therefore  none  available  to  determine  if  arsenic,  lith- 
ium, and  the  phosphate  and  the  borate  radicles  were 
present. 


No.  1,  1913.)     Kelly  and  Ans£acli—Jemez  Plateau  Waters  \ 

ANALYSIS  OF  THE  WATER  FROM  SPRING  No.  11, 

MUD  GEYSER,  SULPHUR  SPRINGS,  N.  M. 

Analysed  by  Mr.  Clyde  Kelly. 


Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO2  , 

356.0 

7.53 

Fe203   1 

518  0 

10  98 

A1203    { 
Ca  

15.2 

0.32 

Mg  . 

18.6 

0.39 

Na    

7.9 

0.16 

K   

32.9 

0.69 

SO4 

3707.0 

78.41 

C03   
HCO3    
Cl    

0.0 
0.0 
8.1 

0.00 
0.00 

0  17 

NO, 

0  0 

0  00 

Aridity     

2724  4 

FLS    .'  
Fe  

63.9 
319.8 

1.35 

Total  Solids  not 
determined. 


*4727.6 


100.00 


*    Acidity  and  total  iron  not  included  in  total. 

Qualitative  tests  on  the  mud  in  the  geyser  showed 
absence  of  arsenic,  lithium,  phosphate  and  borate 
radicles. 

Because  of  the  high  acidity  of  the  water  total  solids 
were  not  determined  on  this  sample. 


40  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

ANALYSIS  OE  THE  WATER  FROM  SPRING  No.  12, 

SELTZER  SPRING,  SULPHUR  SPRINGS,  N.  M. 

Analysed  by  Mr.  Clyde  Kelly. 


Constituents                     Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO2  35.2 

3.14 

Fe203   1 
A1203    \ 
Ca    220  0 

0.93 

IQ  65 

Mg  "  i               48 

0  43 

Na   22.4 

2  00 

K   15.5 

1  39 

SO4                                   589  4 

52  65 

CO,                                      0  0 

0  00 

HCO3                                212  3 

18  97 

Cl    8.1 
NO,  1.3 
Acidity  0.0 
H2S                         i            Trace 

0.72 
0.12 
0.00 

1119.4 
Total  Solids,' 
heated  one 
hour  at  180°C..             972.0 

100.00- 

No  sinter  was  formed  around  this  spring ;  therefore 
none  available  for  determining  the  presence  or  ab- 
sence of  arsenic,  lithium,  and  phosphate  and  borate 
radicles. 


Xo.  1.  1913.)      Kelly  and  Ansjach—Jemez  Plateau  Waters 

ANALYSIS  OF  THE  WATER  FROM  SPRING  No.  13. 

ELECTRIC  SPRING,  SULPHUR  SPRINGS,  N.  M. 

Analysed  by  Mr.  E.  V.  Anspach. 


Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiO,  

186.0 

3.45 

Fe.,6,   1 
A1203    J 
Ca 

953.6 
48  0 

17.69 
0  89 

Me-  . 

1.0 

0.02 

\a 

47  8 

0  8Q 

K 

80  0 

1  48 

SO, 

4061.6 

75.33 

CO.,    

0.0 

0.00 

HCO3    

0.0 

0.00 

Cl  

12.1 

0.22 

NO.. 

1.5 

0.03 

Aciditv   

2587.2 

H2S    ' 

Trace 

Fe    

500.1 

, 

Total  Solids, 
heated   one 
hour  at  110°C.  . 

*5391.6 

5220.0 

100.00       * 

*     Acidity  and  total   iron  not  included  in   total. 

Qualitative  tests  on  the  deposit  of  the  Spring  showed 
the  presence  of  arsenic,  and  the  absence  of  lithium, 
and  the  phosphate  and  bo  rate  radicles. 


42 


Bulletin  University  of  New  Mexico    (Chem.  Ser.,  Vol.  1 


ANALYSIS  OF  THE  WATER  FROM  SPRING  No.  14, 


Analysed  by  Mr.  E.  V.  Anspach. 

Constituents 

Parts  per 
Million 

Per  cent  of 
total  material 
in  solution 

SiOo 

148.0 
1174.0 

141.3  ' 
7.1 
780.8 
34.7 
4989.4 
0.0 
0.0 
8.1 
0.0 
1156.4 
67.7 
206.3 

2.02 
15.97 

1.92 
0.10 
10.62 
0.47 
67.87 
0.00 
0.00 
0.11 
0.00 

0.92 

Fe263   I 
A120,   j 
Ca 

Mg" 

Na       

K   

S04    
CO,   . 

HCO3  

Cl    

NO, 

Acidity  

Fe 

Total  Solids, 
heated  one 
hour  at  110°C.  . 

*8565.8 
7112.5 

100.00 

Acidity  and  total  iron  not  included  in  total. 


No.  1,  1913.)     Kelly  and  Ans^acJi—Jemez  Plateau  Waters  43 

Qualitative  analysis  of  the  mud  from  the  bottom  of 
the  bath-tub  showed  the  presence  of  arsenic,  and  the 
absence  of  lithium ;  also  the  presence  of  the  phosphate 
radicle  and  the  absence  of  the  borate  radicle. 


44  Bulletin  University  of  New  Mexico    (Chem.  Ser.,  Vol.  1 

THE  SOURCE  OF  HEAT 

In  comparing  the  temperatures  of  the  different 
groups  of  springs,  we  find  that  those  situated  nearest 
Mt.  Pelado  have  the  greatest  degree  of  heat,  while 
those  at  the  greatest  distance  from  this  mountain  are 
either  cold  or  nearly  so.  In  other  words,  the  tempera- 
ture decreases  as  the  distance  from  Mt.  Pelado  in- 
creases. Mt.  Pelado,  as  we  know,  was  once  part  of  the 
rim  of  a  great  volcano.  It  is  evident  from  this  that  the 
heat  producing  agent  is  near  the  locality  of  this  vol 
cano.  We  believe  that  there  still  exists,  deep  under- 
ground, a  large  mass  of  heated  rock,  with  which  de- 
scending waters  come  in  contact. 

The  composition  of  the  gas  we  analysed  shows 
that  it  contains  atmospheric  air  as  well  as  carbon  di- 
oxide. This  would  indicate  that  a  part  of  the  water 
had  been  near  the  air  shortly  before  it  came  into  con- 
tact with  the  source  of  heat.  Deep-seated  waters  coin- 
ing into  contact  with  heated  rock  probably  ascend  to- 
ward the  surface  as  vapors.  During  their  ascent  they 
probably  meet  cold  spring  waters  which  are  heated  by 
them.  It  is  interesting  to  note  that  hot  springs  have 
never  been  found  to  exist  in  any  localities  except  where 
igneous  rocks  are  present.  This,  in  itself,  would  seem 
sufficient  to  contradict  any  hypothesis  attempting  to 
assign  the  cause  of  heat  to  chemical  action  alone. 

CHEMISTRY  INVOLVED. 

From  the  foregoing  analyses  we  can  see  that  the 
springs  we  have  analysed  may  be  divided  into  the  fol- 


No.  1,  1913.)     Kelly  and  Ansfach— Jemez  Plateau  Waters  45 

lowing  general  classes  with  respect  to  their  negative 
or  acid  radicles : 

I.     Sulphato-carbonate  waters  SO^  and  CO- 

both  abundant. 

II.     Triple   waters,    containing   chlorides,    sul- 
phites, and     carbonates,     all  in     notable 
amounts. 
III.     Acid  waters,  containing  free  acids.   Acid 

chiefly  sulphuric. 

The  different  classes  will  be  considered  in  the- order 
mentioned  above. 

The  method  of  formation  of  the  different  waters 
is  merely  a  theory  and  not  a  proven  fact ;  and  the  fol- 
lowing are  the  theories  probably  best  fitted  to  the  form- 
ation of  the  waters  of  the  Jemez  Plateau,  since  the 
strata  of  the  region  make  such  theories  possible. 

It  is  evident  that  the  waters  of  the  sulphate-car- 
Ixmate  class  have  primarily  come  up  through  the  Car- 
boniferous strata,  and,  since  sodium  carbonate  and  cal- 
cium sulphate  are  readily  soluble  in  water,  have  dissolved 
a  large  quantity  of  these  alkalies  and  carried  them 
along  in  solution.  Further  on  in  its  course  this  alka- 
line water  has  probably  come  in  contact  with  some  form 
of  granite,  such  as  rhyolite,  and  dissolved  some  of  the 
silica.  This  silica  in  solution  will  then  act  on  a  car- 
bonate producing  a  silicate  and  freeing  carbon  dioxide, 
as  shown  by  the  equation. 

CaCO,     4-     Si02  CaSiO,     +  '  CO2. 

This    would    partly   account    for    the    carbon    dioxide 
coming  from  the     springs,     though  it  is  not  probable 


46  Bulletin  University  of  New  Mexico      ;Chem.  Scr.,  Vol.  1 

that  all  of  the  carbon  dioxide  issuing  from  the  springs 
is  formed  by  this  reaction  alone.  Possibly  some  of  this 
gas  is  formed  by  the  decomposing  of  carbonate  rocks 
by  highly  heated  steam  formed  by  water  coming  in 
contact  with  heated  rocks  deep  under  the  surface  of 
the  earth.  The  carbon  dioxide  may  also  be  obtained 
from  the  bicarbonates  breaking  down  as,  for  example, 

CaCHCOJ,  =  CaC03  4-  H2O  +  CO,. 

TRIPLE  WATERS. 

The  triple  waters  have  probably  been  formed  ex- 
actly as  have  been  the  sulphate-carbonate  waters,  with 
the  one  exception  of  having  come  in  contact  with  a 
strata  of  calcium  or  sodium  chloride. 

ACID  WATERS. 

The  formation  of  sulphuric  acid  in  the  acid  mineral 
waters  has  been  well  explained  by  Mr.  G.  F.  Becker  in 
Monograph  XIII  of  the  U.  S.  Geological  Survey,  pp. 
254-55 : 

"The  formation  of  sulphur  and  sulphuric  acid 
from  hydrosulphuric  acid  by  oxidation  is  one  of 
the  most  familiar  facts  of  chemical  geology  and  of 
experimental  chemistry.  The  relations  of  the  two 
processes  are  readily  seen  from  a  thermo-chemical 
standpoint,  for  the  reaction 

H2S-!-40=H2SO4  liberates  201,500  calories  and 
H2S+  0=H2O+S  liberates  59,100  calories. 

Hence  if  oxygen  is  present  in  excess,  as  it  is  at  the 
surface  of  sulphur  springs  and  in  porous  sinters 


No.  1,  1913.)     Kelly  and  Ansfach— Jemez  Plateau  Waters  47 

partially  saturated  with  solutions  of  hydrosulphu- 
ric  acid,  this  will  simply  be  oxidized  to  sulphuric 
acid.  But  if  oxygen  is  deficient,  as  it  must  be  a 
short  distance  from  the  surface,  a  single  atom  of 
oxygen  by  combining  with  ^H2S  to  54H2SO4 
would  produce  only  50,375  calories,  or  8,725  less 
than  it  sets  free  according  to  the  second  of  the 
above  reactions.  Assuming,  therefore,  that  the 
two  reactions  are  accomplished  in  nearly  the  same 
time,  sulphuric  acid  will  be  formed  at  the  surface 
of  such  a  region  and  free  sulphur  below  the  sur- 
face. This  is  in  correspondence  with  observations 
at  sulphur  springs  the  world  over  and  with  lab- 
oratory experiments.  When,  sulphides  of  the  al- 
kalies are  present  the  reactions  are  more  complex, 
but  sulphur  is  also  separated  while  hyposulphites 
are  formed.  There  is  nothing  strange  or  novel  in 
the  occurrence  of  sulphur  under  the  conditions 
present — ". 

It  is  also  to  be  borne  in  mind  that  aqueous  sulphuric 
acid  will  decompose  chlorides,  with  liberation  of  hy- 
drochloric acid,  and  this  reaction  also  probably  occurs. 
The  acidity  of  a  mineral  water,  then,  may  be  due  to  a 
variety  of  causes,  which  operate  under  varying  condi- 
tions of  material  and  temperature. 

CHANGES   IN    WATERS. 

The  following,  although  not  enclosed  in  quotation 
marks,  is  taken  directly  from  Bulletin  491  of  the  U.  S. 
Geological  survey. 

When  the  water  of  a  spring  emerges  into  the  open 
air  it  begins  to  undergo  changes.  It  may  flow  into 


4g  Bulletin  University  of  New  Mexico      [Chem.  Ser.,  Vol.  1 

other  waters,  and  so  lose  its  individuality ;  it  may  sim- 
ply evaporate,  leaving  a  saline  residue ;  it  may  react 
upon  adjacent  material  and  so  produce  new  substances ; 
or,  by  cooling,  it  may  deposit  some  one  or  more  of  its 
constituents.  The  first  of  these  contingencies  admits 
of  no  systematic  discussion;  the  third  will  be  considered 
in  the  next  chapter;  the  others  can  receive  attention 
now. 

Alteration  by  loss  of  gasequs  contents  is  observed  in 
two  important  groups — the  sulphur  waters  and  those 
containing  an  excess  of  carbonic  acid.  Hydrogen  sul- 
phide partly  escapes  into  the  atmosphere  without  imme- 
diate change,  and  part  of  it  is  oxidized,  with  deposition  of 
sulphur  and  the  formation  of  thiosulphates  and  finally 
sulphates,  which  remain  in  solution.  Deposits  of  finely 
divided  sulphur  are  common  around  those  springs 
which  emit  hydrogen  sulphide,  but  they  frequently  con- 
tain other  substances,  such  as  silica,  calcium  carbonate, 
and  ocherous  matter.  Since,  however,  the  sulphur  is  a 
product  of  partial  oxidation,  this  change  comes  more 
appropriately  under  the  heading  of  reaction  with  ad- 
jacent material,  the  latter  in  this  case,  being  oxygen 
derived  from  the  air.  The  hydrogen  sulphide  itself 
may  be  generated  by  the  action  of  acid  upon  other 
sulphides,  but  it  is  more  commonly  produced  by  the 
reduction  of  sulphates  through  the  agency  of  organic 
matter,  and  the  subsequent  decomposition  of  the  re- 
sultant alkaline  compounds  by  carbonic  acid.  The  last 
reaction,  however,  is  reversible.  Carbon  dioxide  de- 
composes solutions  of  calcium  hydrosulphide ;  but.  on 
the  other  hand,  hydrogen  sulphide  can  partly  decom- 


No.  1,  1913.)       Kelly  and  Ansfach—Jemez  Plateau  Waters  4<) 

pose  solutions  of  calcium  carbonate.  Bicarbonates  and 
sulphides,  therefore,  can  co-exist  in  mineral  waters  in  a 
state  of  unstable  equilibrium. 

CALCAREOUS  SINTER. 

With  carbonated  waters  the  changes  due  to  escape 
of  gas  are  more  conspicuous,  at  least  when  calcium, 
magnesium  or  iron  happen  to  be  the  important  basic 
ions.  When  the  "bicarbonic"  ion  HCO3  breaks  up. 
losing  carbon  dioxide  to  the  atmosphere,  the  normal 
calcium  or  magnesium  carbonate  is  formed  and,  being 
insoluble,  is  precipitated.  If  we  assume  calcium  bicar- 
bonate as  existent  in  solution,  the  reaction  is  as  fol- 
lows : 

CaH,C2Ou  CaCO3     +     H2O     -f     CO2; 

but  the  change  is  modified  by  other  substances  which 
may  be  present,  and  so  the  product  is  rarely  pure,  nor 
is  the  precipitation  absolutely  complete.  Calcareous 
sinter,  Una,  or  travertine  is  thus  produced,  and  in 
many  localities  it  is  an  important  deposit.  The  car- 
bonate waters  of  the  Yellowstone  Park,  for  example, 
form  large  bodies  of  this  character,  and  many  analyses 
of  it  have  been  made. 

The  commonest  companion  of  calcium  carbonate  in 
sinter  is  magnesium  carbonate,  which  is  rarely,  if  ever, 
absent.  The  presence  of  magnesium  salts  in  a  water 
favors  the  deposition  of  calcium  carbonate  in  the  form 
of  aragonite.  Calcite,  however,  is  much  more  common 
in  sinters  than  aragonite.  In  rare  instances  flourite  is 
deposited.  Silica  and  ferric  hydroxide  are  also  fre- 
quent contaminations  of  tufas.  In  short,  the  calcium 


50  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

carbonate  precipitated  from  natural  waters  may  carry 
down  with  it  a  great  variety  of  impurities,  which  de- 
pend upon  the  character  of  the  spring. 

OCHEROUS  DEPOSITS. 

When  ferrous  ions  are  present  in  a  carbonate  water, 
loss  of  carbonic  acid  is  followed  or  accompanied  by 
oxidation,  and  the  precipitated  material  is  an  ocherous 
ferric  hydroxide.  Around  chalybeate  springs  these  de- 
posits of  iron  rust  are  always  noticeable.  With  sub- 
stances of  this  character  calcium  and  magnesium 
carbonates  are  often  thrown  down,  and  also  silica,  so 
that  the  ochers  from  iron  springs  vary  much  in  com- 
position. Between  an  ocher  and  a  calcareous  sinter 
every  intermediate  mixture  may  occur.  Sometimes 
when  sulphates  have  been  reduced  by  organic  matter 
sulphides  of  iron  are  deposited. 

SILICEOUS   DEPOSITS. 

.  Siliceous  deposits  are  formed  by  all  waters  contain- 
ing silica,  but  are  commonly  so  small  as  to  be  incon- 
spicuous. The  silica  then  appears  as  an  impurity  in 
something  else.  From  hot  springs,  however,  which 
often  contain  silica  in  large  quantities,  great  bodies  of 
sinter  are  produced,  and  this  has  a  composition  ap- 
proaching that  of  opal.  Mineralogically,  siliceous  sin- 
ter is  classed  as  a  variety  of  opal,  for  it  consists  mainly 
of  hydrated  silica  with  variable  impurities. 

When  a  water  has  become  sufficiently  concentrated 
to  begin  the  deposition  of  solid  matter,  every  change 
in  concentration  or  temperature  introduces  a  new  set 
,of  conditions  which  determine  the  nature  of  the  com- 


No.  1,  1913.)      Kelly  and  Ansfach— Jemez  Plateau  Waters  §\ 

pounds  to  be  formed.  It  is  clear  from  the  nature  of 
the  products  thus  far  considered,  that  in  a  complex 
water  several  reactions  may  take  place  simultaneously, 
a  number  of  substances  being  thrown  down  at  the 
same  time.  If  water  carrying  much  iron  and  much 
calcium  loses  hydrogen  sulphide  and  carbonic  acid,  then 
ferric  hydroxide,  calcium  carbonate,  and  sulphur  will 
be  deposited  together,  each  change  being  independent 
of  the  others.  In  such  cases  the  complexity  of  reaction 
is  apparent  only,  and  not  real.  The  reactions  are  all 
simple  and  easily  understood.  When  salts  are  formed 
by  evaporation  of  a  water,  the  interpretation  of  the 
phenomena  is  more  difficult. 

REACTIONS    WITH    ADJACENT    MATERIAL. 

The  reactions  of  natural  waters  in  contact  with  ad- 
jacent materials  are  of  many  different  kinds.  We 
have  already  seen  how  oxygen  from  the  atmosphere 
may  convert  ferrous  into  ferric  compounds  and  sul- 
phides into  sulphates,  but  reducing  agents  also  must  be 
taken  into  account.  The  sulphates  of  a  water,  by  ac- 
cession of  organic  matter,  can  be  partly  or  entirely  re- 
duced to  sulphides,  and  carbonic  acid,  acting  upon  the 
latter,  may  expel  sulphureted  hydrogen  and  produce 
carbonates.  By  reaction  of  that  kind  a  water  can  un- 
dergo a  complete  change  of  type  and  pass  from  one 
class  into  another. 

Acid  waters,  especially  when  hot,  act  vigorously  on 
the  substances  with  which  they  come  in  contact,  pro- 
ducing soluble  chlorides  or  sulphates  according  to 
their  character.  Hydrochloric  acid  forms  the  one  set 


52  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

of  salts,  sulphuric  acid  the  other.  The  extent  of  the 
reactions  will  of  course  depend  upon  the  kind  of  ma- 
terial attacked,  for  some  minerals  and  rocks  are  much 
more  soluble  than  others.  The  carbonate  rocks  are 
naturally  the  most  attackable,  but  no  rock  is  entirely 
exempt  from  changes  of  this  order.  When  we  remem- 
ber that  even  pure  and  cold  water  exerts  a  solvent  ac- 
tion upon  many  silicates,  \ve  can  see  how  violently 
corrosive  a  hot,  acid,  volcanic  water  must  be.  Wher- 
ever  waters  of  this  class  occur  the  surrounding  rocks 
are  more  or  less  decomposed,  calcium,  magnesium,  al- 
kalies, and  iron  being  dissolved  out,  while  silica  and 
hydrous  aluminum  silicates  remain  behind.  As  the 
water  cools  and  as  the  acid  becomes  neutralized  its 
activity  decreases,  and  its  peculiar  characteristics  grad- 
ually disappear.  An  ordinary  saline  or  astringent 
water  is  produced  by  these  changes,  which  take  place 
most  rapidly  when  the  active  solutions  are  concentrated 
and  hot,  and  more  slowly  in  proportion  as  they  are  di- 
luted or  cooled. 

Waters  containing  free  sulphuric  or  hydrochloric  acid 
are,  however,  relatively  rare,  and  their  geological  im- 
portance is  small  compared  with  that  of  carbonated 
solutions.  Meteroic  waters  carrying  free  carbonic  acid 
are  probably  the  most  powerful  agents  in  the  solution 
of  rocks,  although  their  chemical  activity  is  neither' 
violent  nor  rapid.  Being  continually  replenished  from 
the  storehouse  of  the  atmosphere,  their  work  goes  on 
unceasingly  over  a  large  portion  of  our  globe.  The 
calcium  which  they  extract  from  rocks  is  carried  by 
rivers  to  the  sea,  and  is  finally  deposited  in  the  form  of 


X o.  1 ,  1 9 1 3 . )      Kelly  and  Ansfacli—Jemez  Plateau  Waters  53 

limestones.  Springs  and  underground  waters  charged 
with  carbonic  acid  exert  the  same  solvent  action,  but 
locally  and  in  different  degree.  Many  springs,  such  as 
the  Jemez  springs  are  so  heavily  loaded  with  carbonic 
acid  that  they  effervesce  when  issuing  into  the  air,  and 
such  waters  are  peculiarly  potent  in  effecting  the  solu- 
tion of  limestones.  By  percolating  waters  of  this  class 
limestone  caverns  are  made,  and  part  of  the  substance 
dissolved  is  redeposited  as  stalactite  or  stalagmite.  In 
reactions  of  this  kind  the  general  character  of  a  water 
is  not  changed;  it  may  be  a  calcium  carbonate  water 
throughout  its  course,  varying  only  in  gaseous  content 
and  in  concentration,  and  its  chemical  effectiveness  is 
shown  by  its  work  as  a  carrier  in  transporting  from  one 
point  to  another  the  material  that  it  has  dissolved. 

Alkaline  waters,  especially  thermal  waters  of  the 
sodium  carbonate  class,  are  also  active  solvents  of 
mineral  substances.  Their  tendency,  however,  is  op- 
posite to  that  of  the  acid  waters,  for  they  dissolve  silica 
rather  than  bases,  and  act  as  precipitants  for  magnesia 
and  lime.  When  solutions  of  calcium  sulphate  and 
sodium  carbonate  are  commingled,  calcium  carbonate 
is  thrown  down  and  an  equivalent  amount  of  sodium 
sulphate  remains  dissolved.  Since  natural  waters  arc 
rarely,  if  ever,  chemically  equivalent,  reactions  of  this 
sort  between  them  are  necessarily  incomplete,  and  the 
blended  solutions  will  contain  one  group  of  ions  in  ex- 
cess over  the  other.  Thus  a  water  of  mixed  type  is 
produced,  but  the  mixture  is  not  an  average  of  the 
I  wo  solutions,  for  part  of  their  original  load  has  been 
removed.  This  is  a  simple  case  of  reaction,  but  it  may 


54  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

be  complicated  in  various  ways,  and  even  reversed. 
For  instance,  a  solution  of  sodium  sulphate  in  presence 
of  free  carbonic  acid  will  dissolve  calcium  carbonate, 
forming  sodium  bicarbonate  and  a  precipitate  of  gyp- 
sum. Mr.  E.  W.  Hilgard,  in  the  American  Journal  of 
Science,  4th  Ser.,  Vol.  2,  1896,  p.  100,  has  investigated 
this  transformation,  and  regards  it  as  the  principal 
source  of  alkaline  carbonate  solutions  in  nature.  Fur- 
thermore, mineral  substances  with  which  alkaline 
waters  come  in  contact  may  be  profoundly  modified. 

Many  mineral  springs  contain  organic  matter,  pre- 
sumably in  the  form  of  the  so-called  humus  acids,  but 
the  influence  exerted  by  these  substances  is  more  pro- 
nounced in  sxvamp  and  river  waters.  Their  supposed 
solvent  action  upon  rocks  and  soils  has  already  been 
noticed,  as  well  as  their  alleged  efficiency  in  retaining 
silica  in  solution. 

Furthermore,  iron  and  alumina  may  be  removed 
from  sulphate  or  chloride  waters  by  the  action  of  lime- 
stones. If  the  iron  is  in  the  ferrous  state,  it  must  first 
be  oxidized  to  the  ferric  condition.7  Then,  by  means 
of  calcium  carbonate,  both  of  the  bases  named  can  be 
precipitated,  either  as  hydroxides  or  as  Msic  sulphates. 
Insoluble  compounds  of  the  latter  class  are  often  formed 
from  natural  waters,  and  many  mineral  species  are  of 
that  character.  It  is  quite  probable  that  limestone  is 
also  effective  in  removing  other  heavy  metals  from 
their  solutions ;  copper,  for  example,  is  certainly  thrown 
down,  but  these  reactions  need  to  be  more  fully  inves- 
tigated. 


Xo.  1,  1913.)     Kelly  and  A nsfacJi— Jemez  Plateau  Waters  55 

Finally,  the  character  of  a  water  may  be  greatly 
changed  by  simple  percolation  through  the  soil.  That 
potassium  is  thus  removed  from  natural  waters  has 
long  been  known.  Hydrous  aluminium  silicates  may  be 
the  effective  absorbents,  or,  in  the  case  of  phosphoric 
acid,  the  hydroxides  of  aluminium  and  iron.  After 
potassium  and  ammonium,  Van  Bemmelen  finds  that 
magnesium  is  most  readily  absorbed,  then  sodium,  and 
calcium  least  of  all.  It  is  clear,  however,  that  the  na- 
ture'of  the  soil  must  be  taken  into  account.  A  sandy 
soil  or  an  impervious  clay  would  be  less  effective  in  re- 
moving saline  substances  from  water  than  a  loose  loam 
rich  in  hydrous  basic  compounds.  The  fact  that  sub- 
stances are  taken  from  waters  by  soils  is  certain,  but  the 
extent  of  the  absorption  depends  upon  local  conditions. 
It  is  also  certain  that  potassium,  rather  than  sodium, 
is  thus  withdrawn  from  aqueous  circulation. 

A  careful  consideration  of  all  the  evidence  concern- 
ing mineral  springs  will  show  that  it  is  exceedingly  dif- 
ficult to  generalize  on  relations  between  the  composi- 
tion of  a  water  and  its  geological  history.  Reactions 
which  take  place  deep  within  the  earth  can  not  easily 
be  traced,  especially  as  a  water  may  undergo  various 
modifications  before  it  reaches  different  sources — 
either  a  direct  mixture  or  a  solution  from  which  ingredi- 
ents have  been  removed — and  it  is  only  in  specific 
cases  that  a  simple  interpretation  of  the  phenomena  can 
be  found.  The  water  that  rises  from  a  salt  bed  or  from 
gypsum  is  easily  understood,  and  so  also  is  one  which 
carries  sulphates  derived  from  pyritiferous  shales.  We 
can  see  that  a  water  from  granite  must  differ  greatly 


^Q  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

from  one  issuing  out  of  limestone.  Many  irregulari- 
ties can  be  traced,  but  no  general  principle  can  be  de- 
duced from  them. 

Various  attempts  have  been  made  to  correlate  the 
composition  of  waters  with  the  geological  horizons 
from  which  they  flow.  For  spring  waters  such  attempts 
are  of  little  value,  because  two  springs,  side  by  side, 
may  be  widely  different.  Artesian  waters  of  common 
origin  often  show  a  family  likeness  to  one  another,  es- 
pecially in  their  minor  constitutents,  one  group  being 
always  calciferous,  another  relatively  rich  in  bromine, 
and  so  on.  But  no  law  can  be  framed  to  cover  even 
these  regularities,  for  the  exceptional  waters  are  too 
numerous  and  too  confusing.  That  waters  from  sed- 
imentary rocks  are,  as  a  rule,  more  concentrated  and 
perhaps  more  complex  than  those  from  the  older  crys- 
talline formations  is  doubtless  true ;  but  beyond  that  it 
is  hardly  safe  to  generalize. 

THERMAL  SPRINGS  AND  VOLCANISM. 

When  a  crystalline  rock,  like  granite,  is  heated  to 
redness  in  vacuo,  water  and  gases,  the  latter  identi- 
cal in  character  with  the  volcanic  ga«es,  are  given  off. 
For  instance,  to  cite  the  least  significant  example,  1 
cubic  kilometer  of  granite  can  yield  from  25  to  30  mil- 
lions of  metric  tons  of  water,  which  at  1,100°  would 
form  160.000,000,000  cubic  meters  of  steam.  In  ad- 
dition to  this  enormous  volume  of  vapor  28,000,000,- 
000  cubic  meters  of  other  gases  would  be  emitted.  Sup- 
pose now  that  by  fissuring  and  subsidence  in  the  litho- 
sphere  such  a  mass  of  rock  were  carried  down  to  a 
depth  of  25,000  to  30,000  meters.  It  would  then  be  in 


No.  1.  1913.)     Kelly  and  Ansfacli—Jemez  Plateau  Waters  57 

the  heated  region,  and  the  evolution  of  vapors  under 
great  pressure  would  occur.  To  some  such  changes 
Gautier  ascribes  the  phenomena  of  volcanism,  with  all 
its  development  of  solfataras  and  fumaroles.  Ordinary 
thermal  springs  may  be  formed  by  the  same  process, 
operating,  perhaps,  less  violently,  and  originate,  so 
to  speak,  from  a  sort  of  distillation  of  the  combined 
water  contained  in  the  depressed  masses  of  rock. 

And  yet.  notwithstanding  all  that  has  been  written 
on  the  subject,  the  controversy  over  the  genesis  of  hot 
springs  is  not  closed.  What  is  the  origin  of  the  carbon 
dioxide  with  which  so  many  mineral  waters  are  heavily 
charged?  In  some  instances,  doubtless,  it  is  derived 
from  the  decomposition  of  limestones,  but  in  others 
this  explanation  cannot  suffice.  Here  and  there  it 
may  be,  to  use  Suess's  expression,  "juvenile,"  and  evi- 
dence of  the  deep-seated  origin  of  the  spring.  Again, 
whence  comes  the  sodium  chloride  of  waters  that  flow 
from  sources  where  it  could  not  have  been  previously 
laid  down?  These  questions,  and  others  like  them, 
still  await  satisfactory  answers.  With  mere  supposi- 
tions, however,  plausible  they  may  seem,  we  cannot  be 
content. 

A  word  in  conclusion  on  the  radioactivity  of  spring 
waters.  A  very  large'  number  of  such  waters  possess 
this  property,  but  no  distinction  between  vadose  and 
juvenile  waters  can  be  based  upon  the  observations. 
Waters  of  both  classes  are  radioactive,  but  the  phe- 
nomenon is  perhaps  most  common  among  waters  of 
volcanic  origin,  or  at  least  among  thermal  springs. 


58  BuJhtfn  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 


CONCLUSION. 

As  our  title  states,  this  investigation  has  been  of 
merely  a  preliminary  nature.  We  have  examined  the 
waters  of  only  a  few  of  the  largest  springs  of  the 
groups  now  being  used  by  white  men.  We  believe 
these  springs  to  be  typical  of  the  groups  in  which  they 
are  located,  however,  and  a  study  of  other  springs  of 
the  same  groups  would  probably  furnish  nothing  more 
than  additional  data  of  a  similar  nature.  A  more  ex- 
tended study  of  the  waters  should  include  an  investi- 
gation of  many  of  the  springs  neglected  by  us,  how- 
ever, for,  although  no  new  conditions  may  be  discov- 
ered, the  data  obtained  would  be  an  additional  check, 
and  would  also  give  more  force  to  the  conclusions 
drawn. 

The  other  groups  rhentioned  in  the  chapter  on  "The 
Springs,"  should  also  be  given  attention  in  an  exhaus- 
tive study  of  the  district.  These  springs,  although  of 
no  importance  commercially  at  present,  could  not  be 
ignored  by  the  scientist  who  seeks  to  unveil  the  geo- 
chemical  secrets  of  the  region. 

As  we  have  intimated  elsewhere  in  this  paper,  the 
most  accurate  methods  of  water  analysis  available 
should  be  employed  if  the  time  at  the  disposal  of  the 
investigator  permits.  In  many  instances,  larger  quan- 
tities of  water  than  we  were  able  to  use  should  be 
taken  for  tTie  determinations.  From  the  analysis  of 
the  sinters  we  have  shown  several  constituents,  which 
we  did  not  determine  in  the  waters,  to  be  present,  in 
small  quantities,  at  least. 


No.  1.  1913.)     Kelly  and  Ansfach— Jemez  Plateau  Waters  59 

The  gas  we  collected  and  analysed  seemed  to  be  a 
typical  example  of  all  that  issuing  from  the  springs  of 
the  Jemez  Hot  Springs  group.  Analyses  of  the  gases 
of  other  groups  should  also  be  made.  Certain  of  the 
elements  of  the  helium  group  may  be  present  in  traces. 

In  his  excellent  booklet  on  the  "Analyses  of  the 
Waters  of  the  Hot  Springs  of  Arkansas,"  Mr.  Hay- 
wood  states  that  the  waters  are  radioactive  in  a  marked 
degree,  and  that  the  salutary  effects  of  the  waters  are 
now  generally  attributed  to  radioactive  substances  in  the 
gaseous  form.  Does  such  a  condition  prevail  in  the 
Jemez  Hot  Springs  ?  This  is  a  bit  of  research  for  some 
later  investigator  to  undertake. 


(50  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 


THE    MEDICINAL    VALUE    OF    THERMAL 
WATERS 

The  curative  effects,  of  thermal  waters  are  un- 
doubtedly due,  to  a  large  extent,  to  their  stimulating 
effect  on  the  excretory  organs  of  the  skin  and  kidneys. 
To  understand  this  fully,  we  have  only  to  examine  the 
routine  through  which  a  patient  passes  at  these  ilitrmal 
resorts.  The  pores  are  first  thoroughly  opei-ed  and 
sweating  begun  by  immersing  the  patient  in  hot  water 
for  from  three  to  ten  minutes.  The  patient  is  then 
placed  in  the  sweating  room  for  about  five  minutes  '.ind 
at  the  same  time  drinks  copiously  of  hot  water.  This 
treatment,  of  course,  produces  profuse  perspiration. 
After  this  the  patient  is  wrapped  in  blankets  and  passed 
to  a  warm  room  for  twenty  to  thirty  minutes  where 
the  perspiration  runs  off  in  streams.  After  this  the 
patient  is  rubbed  down  and  allowed  to  dress.  A  desire 
to  urinate  soon  comes.  Thus  we  see  that  the  system  is 
thoroughly  flooded  with  water  and  washed  out  each 
day,  and  that  tissue  changes  take  place  with  wonderful 
rapidity.  It  is  no  wonder  then  that  the  uric  acid,  syph- 
ilitic poisons,  and  other  materials  of  disease  and  mer- 
curial and  other  metallic  poisons  are  soon  eliminated 
from  the  system.  With  such  effects  as  those  mentioned 
above,  hot  baths  must  be  of  value  in  the  treatment  of 
rheumatism,  gout,  syphillis,  neuralgia,  etc. 


No.  1,1913.)     Kelly  and  Ansfach—Jemez  Plateau  Waters  Q{ 

THE  MEDICINAL  VALUES  OF  THE  VARIOUS 

SALTS  AND  GASES  USUALLY  PRESENT 

IN  MINERAL  WATERS 

The  following  pages  on  the  medicinal  value  of  the 
various  salts  and  gises  usually  found  in  mineral  wa- 
ters have  been  taken  directly  from  Mr.  J.  K.  Hay- 
wood's  "Analyses  of  the  Waters  of  the  Hot  Springs  of 
Arkansas." 

CARBONATES   AND    BICARBONATES. 

One  of  the  most  important  groups  of  mineral  wa- 
ters are  the  alkaline  waters,  which  are  characterized 
by  the  presence,  in  predominating  quantities,  of  one 
or  more  of  the  alkaline  or  alkaline  earth  carbonates. 
These  are  the  carbonates  or  bicarbonates  of  sodium,  po- 
tassium, lithium,  calcium,  and  magnesium.  In  case 
iron  is  present  in  large  quantities  as  the  bicarbonate 
we  have  water  belonging  to  the  chalybeate  class.  Since 
these  waters  are  alkaline  they  are  excellent  remedies  in 
cases  of  sour  stomach  and  in  sick  headaches  which 
arise  from  acid  dyspepsia.  They  act  very  markedly  on 
the  mucous  membranes,  increasing. the  flowr  of  the  gas- 
tric juice  a-cl  other  digestive  fluids,  and  are  conse- 
quently of  use  in  many  cases  of  indigestion.  In  con- 
junction with  the  sulphated  salines  they  give  excellent 
results  when  ir.ed  in  the  treatment  of  catarrhal  con- 
ditions of  the  stomach  and  intestines.  Such  waters 
correct  acidity  of  the  urine,  mirkedly  increase  the  flow 
of  the  urine  and  help  to  dissolve  uric  acid  deposits. 
They  are.  therefore,  of  value  in  cases  of  rheumatism 
and  gout. 


62  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

Sodium  Carbonate  and  Bicarbonate.  Sodium  car- 
bonate or  bicarbonate  appears  as  a  normal  constitu- 
ent of  the  blood,  lymph,  and  nearly  all  secretions  of  the 
mucous  membranes.  Where  conditions  arise  that 
cause  these  fluids  to  become  acid,  waters  containing 
carbonate  and  bicarbonate  of  soda  are  of  value  in  coun- 
teracting the  effect  Waters  containing  either  of  these 
substances  have  been  used  with  excellent  effect  in  the 
treatment  of  acid  dyspepsia  and  diabetes. 

Potassium  Carbonate  and  Bicarbonate.  Potas- 
sium carbonate  and  bicarbonate  are  readily  soluble  in 
water.  The  bicarbonate  is  the  one  usually  present  in 
mineral  waters.  The  properties  of  this  salt  are  very 
much  the  same  as  those  of  sodium  bicarbonate.  It  in- 
creases the  flow  of  urine  and  corrects  acidity  of  the 
bodily  fluids.  . 

Lithium  Carbonate  and  Bicarbonate.  Lithium 
carbonate  is  very  sparingly  soluble  in  water,  while  the 
bicarbonate  is  quite  soluble.  It  is  in  the  latter  form 
that  lithium  is  most  often  reported  in  mineral  waters. 
This  compound  is  most  frquently  used  in  cases  of  rheu- 
matism and  gout,  where  it  forms  a  very  soluble  urate, 
which  is  easily  eliminated  from  the  system. 

Magnesium  Carbonate  and  Bicarbonate.  Mag- 
nesium carbonate  and  bicarbonate  are  mild  laxatives 
and  are  perhaps  the  best  of  all  carbonates  and  bicarbon- 
ates  in  correcting  an  acid  condition  of  the  stomach,  and 
curing  sick  headaches  caused  by  constipation. 

Calcium  Carbonate  and  Bicarbonate.  Calcium  is 
usually  present  in  waters  as  the  bicarbonates.  Both  of 


No.  1,1913.)     Kelly  and  Ansfiacli—Jemez  Plateau  Waters  $3 

these  compounds  are  quite  different  in  their  effects 
from  the  other  carbonates  and  bicarbonates  mentioned. 
While  the  others  are  evacuant  and  promote  secretions, 
the  calcium  compounds  constipate  and  decrease  the  se- 
cretions. Very  obstinate  cases  of  chronic  diarrhea  have 
often  been  cured  by  a  sojourn  at  a  spring  rich  in  cal- 
cium bicarbonate. 

Ferrous  and  Manganous  Bicarbonates.  Neither  iron 
nor  manganese  ever  occurs  in  mineral  waters  as  the 
carbonates,  but  usually  as  the  bicarbonate.  Both  of 
these  compounds  have  practically  the  same  effect. 
When  taken  internally,  they  are  dissolved  by  the  yas- 
tn?  juice  and  taken  into  the  blood.  They  increase  the 
appetite  and  the  number  of  red  blood  corpuscles.  It 
will  thus  be  seen  that  such  waters  give  excellent  re- 
suits  when  used  as  a  tonic  or  in  cases  of  anaemia.  Too 
long  continued  use  of  waters  rich  in  bicarbonate  OF 
iron  or  manganese  results  in  constipation  and  in  de- 
rangement of  the  digestion. 

CHLORIDES. 

Chlorine  occurs  in  waters  as  chlorides,  in  combina- 
tion most  frequently  with  sodium,  potassium  or  lith- 
ium, and  sometimes  with  calcium,  magnesium  or  iron. 
The  chlorides  form  the  basis  of  that  large  group  of 
mineral  waters,  the  muriated  salines. 

Sodium  Chloride.  Sodium  chloride  occurs  in  al- 
most all  mineral  springs  to  some  slight  extent,  but  in 
the  muriated  saline  waters  it  occurs  in  large  quanti- 
ties as  a  predominating  constituent.  Waters  containing 
large  quantities  of  this  substance  are  chiefly  used  in 


g4  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

giving  baths,  which  increase  the  action  of  the  skin,  ami 
by  absorption  through  the  pores  serve  as  a  genuine 
tonic.  Taken  internally  the  flow  of  the  digestive  fluids 
is  promoted  and  the  appetite  increased.  Putrefactive 
changes  in  the  intestines  are  also  prevented.  In  large 
doses  sodium  chloride  increases  the  flow  of  urine  and 
the  amount  of  ir.ea  present  in  the  same. 

Potassium  Chloride.  Potassium  chloride  has  very 
much  the  same  efftct  on  the  human  system  as  does  so- 
dium chloride. 

Lithium  Chloride.  IJthium  chloride  has  practi- 
cally the  same  effect  as  lithium  carbonate  and  bicarbon- 
ate mentioned  above. 

Magnesium  Chloride.  Magnesium  chloride  is 
often  used  medicinally  as  a  cathartic  and  to  increase 
the  flow  of  the  bile. 

Calcium  Chloride.  Calcium  chloride  occurs  in  a 
number  of  muriated  saline  springs.  It  is  used  in  cases 
of  general  debility  as  a  tonic.  It  increases  the  flow  of 
urine  and  per  :p' ration  and  waters  containing  it  are  used 
in  the  treatment  of  scrofulous  diseases  and  eczema. 

Ferrous  Chloride.  The  occurrence  of  ferrous  chlo- 
ride in  mineral  waters  is  rather  rare.  When  present, 
however,  it  acts  as  a  tonic  and  in  general  has  the  same 
effect  as  the  ferrous  bicarbonate  already  mentioned. 

Ammonium  Chloride.  When  used  internally,  am- 
monium chloride  has  the  stimulating  effect  of  am- 
monia. It  is  used  in  nervous  cases  such  as  ovaralgia. 
sciatica,  and  other  neuralgic  disorders.  In  congestion 
of  the  liver  its  use  has  been  beneficial.  Externally  it 


JNo.  1,  1913.)     Kelly  and  Ansfach— Jemez  Plateau  Waters  65 

is  used  as  a  wash  for  ulcers  and  'sores.  It,  however, 
seldom  occurs  in  springs  in  large  enough  quantities  to 
be  of  any  value. 

SULPHATES 

Sulphates  are  frequently  found  in  mineral  waters 
and  when  present  in  large  quantities  give  rise  to  that 
large  class,  the  sulphated  salines. 

Sodium  and  Magnesium  Sulphates.  Sodium  and 
magnesium  sulphates,  or  glauber  and  epsom  salts,  re- 
spectively, in  small  doses  act  as  a  laxative,  in  large 
doses  as  a  cathartic.  They  are  both  valuable  in  in- 
creasing the  flow  of  the  intestinal  fluids  and  in  increas- 
ing the  flow  of  urine  accompanied  by  an  increased  elim- 
ination of  urea.  \Yaters  containing  these  salts  are  of 
great  service  in  eliminating  syphilitic,  scrofulous,  and 
malarial  poisons  of  the  system  and  in  eliminating  mer- 
cury and  other  metallic  poisons.  Persons  suffering 
from  obesitv,  derangement  of  the  liver,  and  Bright's 
disease  are  perhaps  the  most  benefited  by  this  class  of 
waters.  It  must  be  borne  in  mind  that  such  waters 
should  be  used  with  great  care  by  the  feeble  and  an- 
aemic. 

Potassium  Sulphate.  Potassium  sulphate  is  fre- 
quently present  in  mineral  waters,  but  in  smaller  quan- 
tities than  the  magnesium  and  sodium  salts.  Its  action 
is  practically  the  same  as  the  other  two  sulphates  men- 
tioned above. 

Calcium  Sulphate.  Calcium  sulphate  occurs  in  a 
great  many  mineral  waters,  and  is  the  component  that 


66  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

gives  them  the  property  of  permanent  hardness.     It  is 
not  used  medicinally. 

Iron  and  Aluminium  Sulphates.  Iron  and  alumin- 
ium sulphates  are  usually  found  associated  with  each 
other  in  mineral  waters.  They  are  both  partial  astrin- 
gents. The  waters  containing  iron  sulphate  are  also 
used  as  tonics,  but  this  is  not  nearly  as  good  a  form  in 
which  to  give  the  iron  as  is  the  bicarbonate.  Because 
of  their  astringent  action,  waters  containing  these  two 
substances  have  been  used  with  success  in  treating  lo- 
cally inflamed  parts  of  the  mucous  membranes  and  ul- 
cers on  the  outside  of  the  body. 

IODIDES 

The  iodides  are  usually  reported  in  mineral  waters 
as  the  potassium  or  sodium  salt.  They  are  alterative 
in  effect  and  are  consequently  used  in  the  treatment  of 
scrofula,  rheumatism  and  syphilis.  \Yhile  drinking 
waters  containing  iodides  the  flow  of  urine  is  very 
much  increased  and  mercurial  and  other  metallic  pois- 
ons are  rapidly  eliminated  from-  the  system. 

BROMIDES. 

Bromides  act  as  alteratives  in  much  the  same  way 
as  iodides  but  not  to  so  marked  an  effect.  They  also 
act  as  sedatives. 

PHOSPHATES. 

Phosphates  in  mineral  waters  are  usually  reported 
in  one  of  three  forms;  viz.,  sodium,  iron,  or  calcium 
phosphate.  The  sodium  phosphate  acts  as  a  mild  laxn 
tive,  the  iron  phosphate  as  a  tonic,  and  the  calcium 


No.  1,  1913.)     Kelly  and  An^acJt—Jemez  Plateau  Waters  67 

phosphate  as  a  medicine  in  those  conditions  of  the  body 
where  lime  salts  are  deficient,  as  rickets,  etc. 

BORATES 

Boric  acid  is  not  a  very  common  constituent  of 
natural  waters,  but  is  found  as  the  sodium  salt  in 
springs  of  southern  California  in  large  amounts.  Ap- 
plied as  a  douche  in  catarrhal  conditions  of  the  uterus 
it  is  of  value. 

NITRATES 

Any  nitric  acid  that  may  appear  in  any  water  is 
usually  reported  as  sodium  nitrate.  This  compound 
does  not  usually  occur  in  waters  to  a  marked  extent 
unless  they  are  contaminated.  When  present  -in  largo 
enough  amounts  it  increases  the  flow  of  urine  and  acts 
as  a  purgative. 

SILICA. 

Silica  appears  in  mineral  waters  both  as  free  sil- 
ica and  as  silicates.  The  medicinal  value  of  silica  has 
not  been  thoroughly  investigated. 

GASES. 

The  gases  that  usually  occur  in  water  are  nitrogen, 
oxygen,  carbon  dioxide,  and  hydogen  sulphide. 

Nitrogen  and  Oxygen.  Nitrogen  and  oxygen  are 
present  in  all  waters  that  have  come  in  contact  with  the 
air.  On  account  of  the  limited  solubility  of  both  they 
cannot  occur  in  waters  in  very  large  quantities.  Neither 
of  them,  when  present  in  waters,  has  any  medicinal 
value. 


(Jg  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

Carbon  Dioxide.  Carbon  dioxide  is  present  in  all 
natural  waters  to  some  extent,  but  in  some  springs  the 
amount  is  very  large,  thus  giving  rise  to  that  large  class 
of  carbonated  waters  of  which  the  Saratoga  Springs 
furnish  a  good  example.  Such  waters  are  extremely 
palatable  and  large  quantities  can  be  drunk  without  the 
full  feeling,  which  so  often  follows  copious  drinking 
of  water.  In  moderate  quantities  such  waters  increase 
the  flow  of  saliva,  promote  digestion,  and  tend  to  in- 
crease the  flow  of  urine.  Obstinate  cases  of  nausea 
can  be  often  relieved  by  the  use  of  small  quantities  of 
highly  carbonated  waters. 

Hydrogen  Sulphide.  Hydrogen  sulphide  is  pres- 
ent in  many  natural  waters,  giving  to  them  the  odor 
of  decayed  eggs  and  forming  that  large  class,  the  sul- 
phureted  waters.  When  such  waters  are  taken  inter- 
nally they  act  as  an  alterative  and  are  consequently  of 
value  in  the  treatment  of  syphilitic  diseases.  They  in- 
crease the  activity  of  the  intestines,  kidneys,  and  sweat 
glands,  so  are  of  much  use  in  the  treatment  of  rheuma- 
tism and  gout.  Excellent  results  have  been  obtained 
when  these  waters  were  used  in  treating  many  skin  di- 
seases and  malaria. 


No.  1,  1913.)     KeJJy  and  Ansfach—Jemez  Plateau  Waters  QC) 


BIBLIOGRAPHY. 

The  following  literature  will  be  found  useful  for 
reference  under  the  different  phases  of  the  subject  men- 
tioned. 

On  description,  geology  and  physiography  of  the 
Jemcz  Plateau: 

Antiquities  of  the  Jemez  Plateau,  New  Mexico,  by 

Edgar  L.  Hewitt :  Smithsonian  Institution,  Bureau 

of  Ethnology  Bulletin  No.  32. 

American  Geologist,  vol.  31,  No.  2,  Geology  of 

the  Jemez-Albuquerque  Region,  New  Mexico,  by 

A.  B.  Reagan. 

U.  S.  Geographic  Surveys  of  the  Territories,  9th 

annual  report;  monograph  vol.  Ill,  p.  123,  by  Dr. 

Smith. 

Journal  of  Geology,  vol.  VIII,  pp.  448-449. 

On  Methods  of  Analysis  of  Waters: 

Analyses  of  the  Waters  of  the  Hot  Springs  of 
Arkansas,  by  J.  K.  Haywood. 
Analyses  of  the  Waters  of  the  Yellowstone  Na- 
tional Park,  with  an  account  of  the  Methods  of 
Analysis  employed,  by  Frank  Austin  Gooch  and 
James  Edward  Whitfield:  U.  S..  Geological  Sur- 
vey Bulletin  No.  47,  1888. 

Field  Assay  of  Water  by  M.  O.  Leighton,  U.  S. 
Geological  Survey,  Water  Supply  Paper  No.   150. 
Analyses  of  Waters  East  of  the  One  hundredth 


70  Bulletin  University  of  New  Mexico     (Chem.  Ser.,  Vol.  1 

Meridian,  by  R.  B.  Dole,  U.  S.  Geological  Sur- 
vey, Water  Supply  Paper  No.  236,  Part  I. 
Methods   of    Water   Analysis,    published   by   the 
Kennicott    Water    Softener    Company,    Chicago 
Heights,  111. 

On  Analysis  of  Sinters: 

Water-Supply    Investigations    in    Yukon-Tanaria 
Region  Alaska..   1906-1908,  by  C.  C.  Covert  and 
C.  E.  Ellsworth.     U.  S.  Geolo-ical  Survey  Bulle- 
tin No.  228,  p.  323,  pp.  298-299. 
Heilquellen-Analysen,     Dresden,     1885,     by     F. 
Raspe.    A  very  large  collection  of  analyses,  main- 
ly of  European  mineral  waters. 
Geology  of  the  quicksilver  deposits  of  the  Pacific 
Slope;  monograph  U.  S.  Geological  Survey  No. 
XIII. 

American  Journal  of  Science,  3d  series,  vol.  37, 
1889,  p.  351. 

Proc.   Colorado   Scientific   Society,   vol.   8,    1905, 
pp.  1-30. 

.  Allgemeine  und  chemische  Geologic,  vol.    1,  pp. 
599,  600. 

Economic  Geology,  vol.  5,  1910,  p.  22,  analyses 
by  W.  Lindgren. 

The  Data  of  Geochemistry  by  F.  W.  -Clarke.  Bulle- 
tin U.  S.  Geological  Survey,  No.  491. 

Analyses  of  Waters  from  Mineral  Springs: 

Analyses  of  the  Waters  of  the  Hot  Springs  of 
Arkansas  by  J.  K.  Haywood. 
The  Data  of  Geochemistry  by  F.  W.  Clarke,  Bul- 
letin U.  S.  Geological  Survey,  No.  491. 


No.  1,  1913.)     Kelly  and  Ansfiach-Jemez  Plateau  Waters 

Underground  Waters  of  the  Bluegrass  region, 
Kentucky,  by  C.  C.  Matson,  Water  Supply  Paper 
No.  233,  U.  S.  Geological  Survey. 
A  report  of  work  clone  in  the  Washington  labora- 
tory during  the  fiscal  year  1883-84;  F.  W.  Clarke, 
chief  chemist;  Bulletin  U.  S.  Geological  Survey 
No.  9. 

Geology  of  the  Quicksilver  Deposits  of  the  Pacific 
Slope  by  G.  F.  Becker ;  monograph  U.  S.  Geologi- 
cal Survey  No.  XIII. 

A  report  of  work  done  in  the  division  of  chemis- 
try during  the  fiscal  years  1891-92  and  1892-93 ; 
F.  W.  Clarke,  chief  chemist.  Bulletin  U.  S.  Geo- 
logical Survey  No.  113,  p.  114. 
Heil-quellen-Analysen,  Dresden,  1885,  by  F. 
Raspe.  A  very  large  collection  of  analyses,  mainly 
of  European  mineral  waters. 

Dictionary  of  applied  chemistry,  article  "Water," 
vol.  3?  pp.  952-959,  1893,  by  T.  E.  Thorpe.  Ta- 
bles of  analyses  of  European  mineral  springs.  The 
same  article  gives  much  information  about  other 
waters. 

The  mineral  waters  of  the  United  States,  New 
York  and  Philadelphia,  1899,  by  J.  K.  Crook. 
The  mineral  springs  of  the  United  States,  by  A.  C. 
Peak;  Bulletin  U.  S.  Geological  Survey  No.  32, 
1886. 

Analyses  of  the  \Vaters  of  the  Yellowstone  Na- 
tional Park,  by  F.  A.  Gooch  and  J.  E.  Whitfield: 
Bulletin  U.  S.  Geological  Survey  No.  47,  1888. 
Rock  Waters  of  Ohio;  by  E.  Orton:  Nineteenth 


72  Bulletin  University  of  New  Mexico      ^Chem.  Ser.,  Vol.  1 

Annual  Report,  U.  S.  Geological  Survey,  part  4, 
1898,  p.  633.     Contains  many  analyses  of  deep 
wells  from  various  horizons. 
Artesian  wells  of  Iowa,  by  W.  H.  Norton:  Iowa 
Geological  Survey,  vol.  6,' 1896,  pp.  117-428. 
Artesian  wells  of  South  Dakota,  by  J.  H.  Shep- 
herd:  Bulletin  No.  41,  Agricultural   Experiment 
Station  South  Dakota,  1895. 
Mineral  waters  of  Arkansas,  by  J.  C.  Branner: 
Annual     Report     Geological     Survey     Arkansas, 
1891,  vol.  1. 

The  mineral  waters  of  Kansas,  by  E.  H.  S.  Bailey 
and  others :  Kansas  University  Geological  Survev. 
vol.  7,  1902. 

A  report  on  the  mineral  waters  of  Missouri,  by  P. 
Schweitzer :  Geological  Survey  Missouri,  vol.  3. 
1892. 

The  mineral  waters  of  Indiana :  Twenty-sixth  An- 
nual Report  Indiana  Department  Geology  and 
Natural  Resources,  1901,  pp.  11-225.  By  W.  S. 
Blatchley. 

The  mineral  waters  of  lower  Michigan,  by  A.  C. 
Lane :  Water  Supply  Paper  U.  S.  Geological  Sur- 
vey No.  31,  1899. 

Mineral  springs  and  health  resorts  of  California, 
San  Francisco,  1892,  by  W.  Anderson;  contains 
many  analyses,  the  greater  number  of  them  by  the 
author. 

A.  Carnot  and  others.  Analyses  of  French  and 
colonial  mineral  waters  Annales  des  mines,  8th 
ser.,  vol.  7,  1885,  p.  79;  9th  ser.,  vol.  6,  1894, 


No.  1,  1913.)      Kelly  and  Ansfach  -Jemez  Plateau  Waters 

p.  355;  vol.  16,  1899,  p.  33.  These  three  papers 
contain  584  analyses. 

Report  of  the  Australasian  Association  for  the 
Advancement  of  Science,  1898,  hy  L.  Litersidge, 
W.  Skey,  and  G.  Gray;  pp.  87-108.  A  collection 
of  analyses  of  Australasian  mineral,  waters. 
Deutsches  Baderbuch.  Leipzig,  1907.  A  com- 
pendium of  information  relative  to  the  mineral 
springs  of  Germany. 

United  States  Department  of  Agriculture,  Bureau 
of  Chemistry,  Bulletins  91  and  139.  Contain 
many  analyses  of  American  mineral  waters. 

Analyses  of  H'atcrs  of  the  Jeniec  Plateau: 

Loew,  Analysis  of  mineral  springs,  Vol.  Ill,  U.  S 
Geographic  Surveys  of  the  Territories. 
Lists  and  analyses  of  the  mineral  springs  of  the 
United  States  (a  preliminary  study),  by  A.  C. 
Peale,  1896.  Bulletin  U.  S.  Geological  Survey 
No.  32,  p.  193. 

Methods  of  Analysis  of  Gas: 
Hempel,  "Gas  Analysis." 

Medicinal  1'alite  of  Mineral  il'aters: 

Analyses  of  the  Waters  of  the  Hot  Springs  of  Ar- 
kansas, by  J.  K.  Haywood.  Bulletin  Department 
of  the  Interior.  1912. 

Mineral  springs  of  the  United  States  and  Canada, 
by  G.  E.  Walton. 


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